Course Information

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (plus extra credits for completion). Type of Completion: zk (examination).
In-person direct teaching

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 16:00–17:50 B11/335

Prerequisites

NOW( C3110 Analytical Chemistry I-sem. )
The prerequisite is the completion of basic lectures from General Chemistry (C1020) and the relevant laboratory exercises from this subject.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 6 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing information from the course, he can also analyse problems and propose solutions.

Learning outcomes

Students will get acquainted with the basics of analytical chemistry, qualitative analysis and methods of gravimetric and volumetric analysis

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyte, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and its determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, thermogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems associated with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination of Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration of Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems associated with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside and diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and its titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

required literature
• SKOOG, Douglas A., Donald M. WEST, F. James HOLLER and Stanley R. CROUCH. Analytická chemie. Translated by Karel Nesměrák - Václav Červený - Tomáš Křížek - Eliška. Vydání první. Praha: Vysoká škola chemicko-technologická v Praze, 2019, xxx, 950. ISBN 9788075920430. info

recommended literature
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info

not specified
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001

Teaching methods

lectures

Assessment methods

2 h lecture
written examination

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further comments (probably available only in Czech)

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 15:00–16:50 B11/335

Prerequisites

NOW( C3110 Analytical Chemistry I-sem. )
The prerequisite is the completion of basic lectures from General Chemistry (C1020) and the relevant laboratory exercises from this subject.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 6 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing information from the course, he can also analyse problems and propose solutions.

Learning outcomes

Students will get acquainted with the basics of analytical chemistry, qualitative analysis and methods of gravimetric and volumetric analysis

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyte, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and its determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, thermogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems associated with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination of Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration of Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems associated with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside and diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and its titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

required literature
• SKOOG, Douglas A., Donald M. WEST, F. James HOLLER and Stanley R. CROUCH. Analytická chemie. Translated by Karel Nesměrák - Václav Červený - Tomáš Křížek - Eliška. Vydání první. Praha: Vysoká škola chemicko-technologická v Praze, 2019, xxx, 950. ISBN 9788075920430. info

recommended literature
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info

not specified
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001

Teaching methods

lectures

Assessment methods

2 h lecture
written examination

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further comments (probably available only in Czech)

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Mon 14:00–15:50 B11/205

Prerequisites

NOW( C3110 Analytical Chemistry I-sem. )
The prerequisite is the completion of basic lectures from General Chemistry (C1020) and the relevant laboratory exercises from this subject.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 6 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing information from the course, he can also analyse problems and propose solutions.

Learning outcomes

Students will get acquainted with the basics of analytical chemistry, qualitative analysis and methods of gravimetric and volumetric analysis

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyte, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and its determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, thermogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems associated with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination of Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration of Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems associated with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside and diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and its titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

required literature
• SKOOG, Douglas A., Donald M. WEST, F. James HOLLER and Stanley R. CROUCH. Analytická chemie. Translated by Karel Nesměrák - Václav Červený - Tomáš Křížek - Eliška. Vydání první. Praha: Vysoká škola chemicko-technologická v Praze, 2019, xxx, 950. ISBN 9788075920430. info

recommended literature
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info

not specified
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001

Teaching methods

lectures

Assessment methods

2 h lecture
written examination

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further comments (probably available only in Czech)

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 17:00–18:50 B11/306

Prerequisites

NOW( C3110 Analytical Chemistry I-sem. )
The prerequisite is the completion of basic lectures from General Chemistry (C1020) and the relevant laboratory exercises from this subject.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 6 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing information from the course, he can also analyse problems and propose solutions.

Learning outcomes

Students will get acquainted with the basics of analytical chemistry, qualitative analysis and methods of gravimetric and volumetric analysis

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyte, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and its determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, thermogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems associated with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination of Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration of Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems associated with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside and diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and its titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

required literature
• SKOOG, Douglas A., Donald M. WEST, F. James HOLLER and Stanley R. CROUCH. Analytická chemie. Translated by Karel Nesměrák - Václav Červený - Tomáš Křížek - Eliška. Vydání první. Praha: Vysoká škola chemicko-technologická v Praze, 2019, xxx, 950. ISBN 9788075920430. info

recommended literature
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info

not specified
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001

Teaching methods

lectures

Assessment methods

2 h lecture
written examination

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further comments (probably available only in Czech)

The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 15:00–16:50 B11/335

Prerequisites

NOW( C3110 Analytical Chemistry I-sem. )
The prerequisite is the completion of basic lectures from General Chemistry (C1020) and the relevant laboratory exercises from this subject.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 6 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing information from the course, he can also analyse problems and propose solutions.

Learning outcomes

Students will get acquainted with the basics of analytical chemistry, qualitative analysis and methods of gravimetric and volumetric analysis

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyte, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and its determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, thermogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems associated with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination of Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration of Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems associated with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside and diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and its titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

required literature
• SKOOG, Douglas A., Donald M. WEST, F. James HOLLER and Stanley R. CROUCH. Analytická chemie. Translated by Karel Nesměrák - Václav Červený - Tomáš Křížek - Eliška. Vydání první. Praha: Vysoká škola chemicko-technologická v Praze, 2019, xxx, 950. ISBN 9788075920430. info

recommended literature
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info

not specified
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001

Teaching methods

lectures

Assessment methods

2 h lecture
written examination

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further comments (probably available only in Czech)

The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 14:00–15:50 B11/335

Prerequisites

NOW( C3110 Analytical Chemistry I-sem. )
The prerequisite is the completion of basic lectures from General Chemistry (C1020) and the relevant laboratory exercises from this subject.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 6 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing information from the course, he can also analyse problems and propose solutions.

Learning outcomes

Students will get acquainted with the basics of analytical chemistry, qualitative analysis and methods of gravimetric and volumetric analysis

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyte, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and its determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, thermogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems associated with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination of Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration of Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems associated with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside and diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and its titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info

Teaching methods

lectures

Assessment methods

2 h lecture
written examination

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further comments (probably available only in Czech)

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Mon 17. 9. to Fri 14. 12. Tue 14:00–15:50 B11/205

Prerequisites (in Czech)

NOW( C3110 Analytical Chemistry I-sem. )
Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 6 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing information from the course, he can also analyse problems and propose solutions.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyte, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and its determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, thermogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems associated with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination of Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration of Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems associated with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside and diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and its titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

recommended literature
• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• ZÁRUBA, Kamil. Analytická chemie. Vydání první. Praha: Vysoká škola chemicko technologická v Praze, 2016, 221 stran. ISBN 9788070809518. info
• ZÁRUBA, Kamil. Analytická chemie. Vydání první. Praha: Vysoká škola chemicko technologická v Praze, 2016, 224 stran. ISBN 9788070809501. info

not specified
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info

Teaching methods

lectures

Assessment methods

2 h lecture
combined exam (written and oral part)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further comments (probably available only in Czech)

The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Mon 18. 9. to Fri 15. 12. Tue 14:00–15:50 B11/205

Prerequisites (in Czech)

NOW( C3110 Analytical Chemistry I-sem. )
Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 6 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing information from the course, he can also analyse problems and propose solutions.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyte, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and its determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, thermogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems associated with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination of Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration of Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems associated with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside and diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and its titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info

Teaching methods

lectures

Assessment methods

2 h lecture
combined exam (written and oral part)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further comments (probably available only in Czech)

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Mon 19. 9. to Sun 18. 12. Tue 14:00–15:50 B11/205

Prerequisites (in Czech)

NOW( C3110 Analytical Chemistry I-sem. )
Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 6 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing information from the course, he can also analyse problems and propose solutions.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyte, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and its determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, thermogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems associated with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination of Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration of Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems associated with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside and diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and its titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info

Teaching methods

lectures

Assessment methods

2 h lecture
combined exam (written and oral part)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further comments (probably available only in Czech)

The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 14:00–15:50 B11/205

Prerequisites (in Czech)

NOW( C3110 Analytical Chemistry I-sem. )
Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 6 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing information from the course, he can also analyse problems and propose solutions.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyte, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and its determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, thermogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems associated with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination of Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration of Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems associated with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside and diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and its titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info

Teaching methods

lectures

Assessment methods

2 h lecture
combined exam (written and oral part)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further comments (probably available only in Czech)

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Mon 9:00–10:50 B11/132

Prerequisites (in Czech)

NOW( C3110 Analytical Chemistry I-sem. )
Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 6 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing information from the course, he can also analyse problems and propose solutions.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyte, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and its determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, thermogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems associated with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination of Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration of Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems associated with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside and diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and its titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info

Teaching methods

lectures

Assessment methods

2 h lecture
combined exam (written and oral part)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further comments (probably available only in Czech)

The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 16:00–17:50 B11/205

Prerequisites (in Czech)

NOW( C3110 Analytical Chemistry I-sem. )
Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 6 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing information from the course, he can also analyse problems and propose solutions.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyte, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and its determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, thermogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems associated with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination of Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration of Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems associated with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside and diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and its titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info

Teaching methods

lectures

Assessment methods

2 h lecture
combined exam (written and oral part)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science
Supplier department: Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Wed 10:00–11:50 B11/132

Prerequisites (in Czech)

NOW( C3110 Analytical Chemistry I-sem. )
Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 6 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing informations from the course, he can also analyse problems and propose solutions.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info

Teaching methods

lectures

Assessment methods

2 h lecture
combined exam (written and oral part)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Wed 10:00–11:50 B11/132

Prerequisites (in Czech)

NOW( C3110 Analytical Chemistry I-sem. )
Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 7 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing informations from the course, he can also analyse problems and propose solutions.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info

Teaching methods

lectures

Assessment methods

2 h lecture
combined exam (written and oral part)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Wed 10:00–11:50 B11/132

Prerequisites (in Czech)

Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 15 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing informations from the course, he can also analyse problems and propose solutions.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info

Teaching methods

lectures

Assessment methods

2 h lecture
combined exam (written and oral part)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Přemysl Lubal, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Fri 11:00–12:50 G2,02003

Prerequisites (in Czech)

Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 17 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing informations from the course, he can also analyse problems and propose solutions.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info

Teaching methods

lectures

Assessment methods

2 h lecture
combined exam (written and oral part)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Přemysl Lubal, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 14:00–15:50 F1 6/1014

Prerequisites (in Czech)

Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 17 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info

Assessment methods

2 h lecture
combined exam (written and oral part)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Přemysl Lubal, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 14:00–15:50 F1 6/1014

Prerequisites (in Czech)

Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 17 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• JANČÁŘ, Luděk and Irena JANČÁROVÁ. Analytická chemie (Analytical Chemistry). první, 2003. MZLU Brno: MZLU Brno, 2003, 195 pp. ISBN 80-7157-647-6. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• SKOOG, Douglas A. Analytical chemistry :an introduction. 7th ed. Fort Worth: Saunders College Publishing, 1999, xxiv, 773. ISBN 0-03-020293-0. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Kellner R., Mermet J.-M., Otto M., Widmer H. M., Analytical Chemistry, Wiley 1998.

Assessment methods (in Czech)

2 hodinová přednáška
kombinovaná zkouška (písemná a ústní část)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Přemysl Lubal, Ph.D. (lecturer)
prof. RNDr. Josef Havel, DrSc. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science

Timetable

Tue 13:00–14:50 02004

Prerequisites (in Czech)

Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 17 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• JANČÁŘ, Luděk and Irena JANČÁROVÁ. Analytická chemie (Analytical Chemistry). první, 2003. MZLU Brno: MZLU Brno, 2003, 195 pp. ISBN 80-7157-647-6. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• SKOOG, Douglas A. Analytical chemistry :an introduction. 7th ed. Fort Worth: Saunders College Publishing, 1999, xxiv, 773. ISBN 0-03-020293-0. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Kellner R., Mermet J.-M., Otto M., Widmer H. M., Analytical Chemistry, Wiley 1998.

Assessment methods (in Czech)

2 hodinová přednáška
kombinovaná zkouška (písemná a ústní část)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

Study Materials
The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Josef Havel, DrSc. (lecturer)
prof. RNDr. Přemysl Lubal, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Chemistry Section – Faculty of Science

Timetable

Thu 11:00–12:50 02004

Prerequisites (in Czech)

Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 17 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• SKOOG, Douglas A. Analytical chemistry :an introduction. 7th ed. Fort Worth: Saunders College Publishing, 1999, xxiv, 773. ISBN 0-03-020293-0. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Kellner R., Mermet J.-M., Otto M., Widmer H. M., Analytical Chemistry, Wiley 1998.

Assessment methods (in Czech)

2 hodinová přednáška
kombinovaná zkouška (písemná a ústní část)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Josef Havel, DrSc. (lecturer)
prof. RNDr. Přemysl Lubal, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Josef Havel, DrSc.
Chemistry Section – Faculty of Science

Timetable

Wed 12:00–13:50 02004

Prerequisites (in Czech)

Předpokladem je absolvování základních přednášek z Obecné chemie (C1020), Anorganické chemie I (C1061), Anorganické chemie II (C2062), Organické chemie I (C2021), Organické chemie II (C3022) a příslušných laboratorních cvičení z těchto předmětů.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 18 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry.

Syllabus

• I. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination.
• 1. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 2. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 3. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 4. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 5. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 6. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 7. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 8. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 9. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 10. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 11. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates.

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• SKOOG, Douglas A. Analytical chemistry :an introduction. 7th ed. Fort Worth: Saunders College Publishing, 1999, xxiv, 773. ISBN 0-03-020293-0. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Kellner R., Mermet J.-M., Otto M., Widmer H. M., Analytical Chemistry, Wiley 1998.

Assessment methods (in Czech)

2 hodinová přednáška
kombinovaná zkouška (písemná a ústní část)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

The course can also be completed outside the examination period.
The course is taught annually.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Josef Havel, DrSc. (lecturer)
prof. RNDr. Přemysl Lubal, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Josef Havel, DrSc.
Chemistry Section – Faculty of Science

Prerequisites (in Czech)

Předpokladem je absolvování základních přednášek z Obecné chemie (C1020), Anorganické chemie I (C1061), Anorganické chemie II (C2062), Organické chemie I (C2021), Organické chemie II (C3022) a příslušných laboratorních cvičení z těchto předmětů.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 18 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry.

Syllabus

• I. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination.
• 1. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 2. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 3. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 4. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 5. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 6. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 7. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 8. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 9. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 10. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 11. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates.

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• SKOOG, Douglas A. Analytical chemistry :an introduction. 7th ed. Fort Worth: Saunders College Publishing, 1999, xxiv, 773. ISBN 0-03-020293-0. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Kellner R., Mermet J.-M., Otto M., Widmer H. M., Analytical Chemistry, Wiley 1998.

Assessment methods (in Czech)

2 hodinová přednáška
kombinovaná zkouška (písemná a ústní část)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

The course can also be completed outside the examination period.
The course is taught annually.
The course is taught: every week.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Josef Havel, DrSc. (lecturer)
prof. RNDr. Přemysl Lubal, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Josef Havel, DrSc.
Chemistry Section – Faculty of Science

Prerequisites (in Czech)

Předpokladem je absolvování základních přednášek z Obecné chemie (C1020), Anorganické chemie I (C1061), Anorganické chemie II (C2062), Organické chemie I (C2021), Organické chemie II (C3022) a příslušných laboratorních cvičení z těchto předmětů.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 18 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry.

Syllabus

• I. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination.
• 1. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 2. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 3. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 4. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 5. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 6. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 7. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 8. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 9. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 10. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 11. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates.

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• SKOOG, Douglas A. Analytical chemistry :an introduction. 7th ed. Fort Worth: Saunders College Publishing, 1999, xxiv, 773. ISBN 0-03-020293-0. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Kellner R., Mermet J.-M., Otto M., Widmer H. M., Analytical Chemistry, Wiley 1998.

Assessment methods (in Czech)

2 hodinová přednáška
kombinovaná zkouška (písemná a ústní část)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

The course can also be completed outside the examination period.
The course is taught annually.
The course is taught: every week.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Josef Havel, DrSc. (lecturer)
prof. RNDr. Přemysl Lubal, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Josef Havel, DrSc.
Chemistry Section – Faculty of Science

Prerequisites (in Czech)

Předpokladem je absolvování základních přednášek z Obecné chemie (C1020), Anorganické chemie I (C1061), Anorganické chemie II (C2062), Organické chemie I (C2021), Organické chemie II (C3022) a příslušných laboratorních cvičení z těchto předmětů.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 18 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry.

Syllabus

• I. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination.
• 1. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 2. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 3. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 4. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 5. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 6. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 7. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 8. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 9. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 10. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 11. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates.

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• SKOOG, Douglas A. Analytical chemistry :an introduction. 7th ed. Fort Worth: Saunders College Publishing, 1999, xxiv, 773. ISBN 0-03-020293-0. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Kellner R., Mermet J.-M., Otto M., Widmer H. M., Analytical Chemistry, Wiley 1998.

Assessment methods (in Czech)

2 hodinová přednáška
kombinovaná zkouška (písemná a ústní část)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

The course can also be completed outside the examination period.
The course is taught annually.
The course is taught: every week.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Josef Havel, DrSc. (lecturer)
prof. RNDr. Přemysl Lubal, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Josef Havel, DrSc.
Chemistry Section – Faculty of Science

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 18 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry.

Language of instruction

Czech

Further Comments

The course can also be completed outside the examination period.
The course is taught annually.
The course is taught: every week.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/1/0. 3 credit(s). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Josef Havel, DrSc. (lecturer)
prof. RNDr. Přemysl Lubal, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Josef Havel, DrSc.
Chemistry Section – Faculty of Science

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 18 fields of study the course is directly associated with, display

Syllabus

• A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry.

Language of instruction

Czech

Further Comments

The course is taught annually.
The course is taught: every week.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

The information about the term Autumn 2011 - acreditation is not made public

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science

Prerequisites (in Czech)

Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 15 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing informations from the course, he can also analyse problems and propose solutions.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info

Teaching methods

lectures

Assessment methods

2 h lecture
combined exam (written and oral part)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

The course can also be completed outside the examination period.
The course is taught annually.
The course is taught: every week.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Viktor Kanický, DrSc. (lecturer)
prof. Mgr. Jan Preisler, Ph.D. (lecturer)
doc. Mgr. Tomáš Vaculovič, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science

Prerequisites (in Czech)

Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 15 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry. On the base of acquired knowledge student is able to understand basic principles of classic analytical chemistry. Utilizing informations from the course, he can also analyse problems and propose solutions.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• HOLZBECHER, Záviš and Jaroslav CHURÁČEK. Analytická chemie. 1. vyd. Praha: Státní nakladatelství technické literatury, 1987, 663 s. info
• Analytical chemistry : a modern approach to analytical science. Edited by Jean-Michel Mermet - Matthias Otto - M. Valcárcel Cases. 2nd ed. Weinheim: Wiley-VCH, 2004, xxviii, 11. ISBN 3527305904. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• SKOOG, Douglas A. Fundamentals of analytical chemistry. 8th ed. Belmont, Calif.: Brooks/Cole, 2004, 1 sv. ISBN 0534417965. info
• CHRISTIAN, Gary D. Analytical chemistry. 6th ed. Hoboken, NJ: John Wiley & Sons, 2003, xix, 828 s. ISBN 0-471-21472-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Enke Ch., The Art and Science of Chemical Analysis, Wiley New York 2001
• OKÁČ, Arnošt. Analytická chemie kvalitativní. 3., dopl. vyd. Praha: Academia, 1966, 573 s. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info

Teaching methods

lectures

Assessment methods

2 h lecture
combined exam (written and oral part)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

The course can also be completed outside the examination period.
The course is taught annually.
The course is taught: every week.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

C3100 Analytical Chemistry I

Extent and Intensity

2/0/0. 2 credit(s) (fasci plus compl plus > 4). Type of Completion: zk (examination).

Teacher(s)

prof. RNDr. Přemysl Lubal, Ph.D. (lecturer)

Guaranteed by

prof. RNDr. Viktor Kanický, DrSc.
Department of Chemistry – Chemistry Section – Faculty of Science

Prerequisites (in Czech)

Předpokladem je absolvování základních přednášky z Obecné chemie (C1020)a příslušného laboratorního cvičení z tohoto předmětu.

Course Enrolment Limitations

The course is also offered to the students of the fields other than those the course is directly associated with.

fields of study / plans the course is directly associated with

there are 17 fields of study the course is directly associated with, display

Course objectives

A systematic treatment of the basic principles of analytical chemistry for students of chemistry - part I. The course includes qualitative analysis, gravimetric analysis, and titrimetry.

Syllabus

• 1. Introduction into subject Analytical chemistry. Definition of basic terms. Definition of analytical chemistry a its position in chemistry and society. Terms: sample, analyt, matrix, method sensitivity. Standards and reference materials. Sampling, analytical methods and procedures. Foundations of Good Laboratory Practice (GLP) and analysis evaluation. Standard deviation of analysis and their determination. Statistical evaluation of analytical results (Gauss, Dean-Dixon and Student test). Rejection of outliers. Definition and parameters for precision and accuracy of analytical method.
• 2. Protolytic reactions in aqueous solutions : acids, bases, water as solvent, autoprotolysis of solvent, constants, calculations of proton concentration in solutions of acids, bases and salts, graphical description of acid-base equilibria.
• 3. Complex formation equilibria : stepwise formation of complexes in solutions, graphical and numerical description of complex formation equilibria, equilibrium constants and stability constants, examples of complex formation equilibria (complexes of ammonia, cyanide, thiocyanate, iodide), cation and anion hydrolysis, chelates of metals and non-metals, organic analytical reagents. Side equilibria in solutions, conditional stability constants and their analytical importance.
• 4. Precipitation reactions : solubility and solubility product, conditional solubility product - influence of side reactions in solutions, substitution precipitation, converse of precipitates, examples of low soluble hydroxides, sulphides, sulphates, halides, chromates, oxalates, 8-hydroxychinolinates, etc.
• 5. Redox equilibria : description of redox reactions and the types, standard and conditional potential, influence of formation of precipitates and complexes in solution, influence of pH, redox disproportionation, examples of oxidising and reducing agents in aqueous solutions.
• 6. Principles of quantitative inorganic chemical analysis. Group and selective reactions. Examples of group precipitating agents, group reduction and oxidation, group characterisation of anions. Selective agents, origin of analytical selectivity. Importance of masking of element ions, masking agents.
• 7. Gravimetry. Processes during precipitation and their influence on gravimetric analysis, contamination of precipitates, processes on precipitates, analytical balance and weighing, some basic operations in gravimetry : filtration and filter washing, drying, ignition, termogravimetry, examples of gravimetric procedures : methods based on AgCl, BaSO4, and hydroxide formation, SiO2 determination, organic agents in gravimetry, precipitation from homogenous solutions, gravimetric calculations, errors in gravimetric determination.
• 8. Titration methods (volumetric analysis). Kinds of titrations, explanation of titration curves of all titration types, relation between inflection point (end of titration) and equivalence point, slope of curve and buffer range, titration calculations, primary standards in volumetry, evaluation of characteristic points on curves. Basic operations and aids in volumetry.
• 9. Precipitation titrations. Explanation of titration curves, estimate of equivalence point, problems joined with indication of equivalence point, titration solutions and primary standards, origin of titration errors. Argentometric titrations : titration curves and their interpretation, interpretation of logarithmic diagrams during precipitation of AgCl, AgBr, AgI, Ag2CrO4, titration curves of mixtures Cl-, Br-, I-; titration errors for each equivalence point, determination Ag+ by NaCl solution without indicator, titration in presence of chromate as indicator, titration in presence of adsorption indicator, titration Ag+ by SCN- solution a indirect Br-, I-, SCN- determination, argentometric titration in presence of redox indicator; iodide titration by Ag+ solution in presence of (I2 + starch). Titration of sulphate by Ba(ClO4)2 solution using sulfonazo III indicator.
• 10. Acid-base titration. Explanation of titration curve, characteristic regions, pH calculation of equivalence point. Titration curves of strong and weak acids and bases; acid-base buffer solutions, capacity (buffer index) and limits of buffer system, suitable buffer solutions for different pH regions, one-colour and two-colour indicators, mixed and fluorescence indicators. Examples of alkalimetric titrations: determination of strong, weak, concentrated acids, HF, B(OH)3, NH4+, alfa-aminoacids; titration of polyprotic acids; buffer capacity of hydrogensalts; determination of oxalic and phosphoric acids; pH estimate of equivalence titration point, calculation of titration error.
• 11. Complexometric titrations. Requirements for complex formation reaction used in titration. Argentometric titration of cyanide : explanation of titration curve, problems joined with equivalence point evaluation (Liebig, Denigés). Mercurimetric determination of halides, thiocyanates, cyanides : explanation of titration curve, indication of equivalence titration point using nitroprusside a diphenylcarbohydrazone. Determination of Hg2+ using SCN- solution. Chelatometric titration : survey of currently used chelating agents, EDTA - titration; explanation of titration curves and determination of characteristic regions of titration curves; influence of conditional stability constants on curve shape; titration curve span and slope of titration curves, criteria for the choice of suitable pH for titration, equivalence point indicators, metallochromic indicators and their functional transitions, mechanism of equivalence point indication using currently used indicators (eriochrom black T, murexide, fluorexon); examples of EDTA titrations, determination of Mg(II) a Ca(II), determination of water hardness, EDTA titration using xylenole orange indicator, possibilities of simultaneous determination of two metal ions, titration solutions, standardization, errors of chelatometric titrations.
• 12. Redox titrations. Explanation of titration curve, characteristic ranges, calculation of potential of equivalence point, conditions for quantitative course of reaction, choice of suitable redox systems taken from redox potentials and equilibrium constants, coupled redox systems, primary titration standards, reversible and irreversible redox indicators, explanation of reaction mechanism of redox indicators, errors of redox titrations. Oxidimetry with KMnO4 solution in acidic medium : stepwise reduction of permanganate, kinetics of reduction, Mn(II) autocatalysis and influence of medium, determination of oxalic acid, oxalates, Ca(II), Fe(II), hydrogen peroxide. Oxidimetry with KMnO4 solution in slightly acidic and alkaline medium, Mn(II) determination.
• 12. Oxidimetry with iodine solution: mechanism of equivalence point indication, determination of sulphites, SO2, H2S, As(III), formaldehyde. Iodide oxidation to iodine and their titration by thiosulphate solution : hydrogen peroxide determination, oxygen in water, Cu(II), Mn(II), chromate, halogens, active chlorine. Analytical use of the system iodate + iodide. Amplification reactions. Oxidimetry with Ce(IV) solution: equivalence point indication; determination of Fe(II), hydrogen peroxide, iodide, oxalic acid, As(III). Oxidimetry with K2Cr2O7 solution : equivalence point indication, determination of Fe(II), ethanol in blood. Oxidimetry with KBrO3 solution: equivalence point indication; determination of As(III), Sb(III), organic compounds; indirect aluminium determination in 8-hydroxychinoline chelates. Reduktometry (titanometry).

Literature

• Sommer L., Základy analytické chemie I, VUTium Brno 1998.
• JANČÁŘ, Luděk and Irena JANČÁROVÁ. Analytická chemie (Analytical Chemistry). první, 2003. MZLU Brno: MZLU Brno, 2003, 195 pp. ISBN 80-7157-647-6. info
• JANČÁŘOVÁ, Irena and Luděk JANČÁŘ. Základní chemické výpočty. Brno: MZLU, 2005, 116 pp. ISBN 80-7157-575-5. info
• ŠENKÝŘ, Jaroslav. Kvalitativní analýza : vybrané postupy k důkazu iontů. 2. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 76 s. ISBN 8021011726. info
• Analytická příručka. Díl I [Zýka, 1988]. Edited by Jaroslav Zýka. 4. upr. vyd. Praha: SNTL - Nakladatelství technické literatury, 1988, 678 s. info
• SOMMER, Lumír. Teoretické základy analytické chemie. I. Brno: Vysoké učení technické, 1995. info
• ŠENKÝŘ, Jaroslav. Kvantitativní analýza : pracovní návody pro základní cvičení. 1. vyd. Brno: Vydavatelství Masarykovy univerzity, 1995, 44 s. ISBN 8021012145. info
• SKOOG, Douglas A. Analytical chemistry :an introduction. 7th ed. Fort Worth: Saunders College Publishing, 1999, xxiv, 773. ISBN 0-03-020293-0. info
• HARRIS, Daniel C. Quantitative chemical analysis. 4th ed. New York: W.H. Freeman, 1995, xix, 837 s. ISBN 0-7167-2508-8. info
• Schwedt Georg, The Essential Guide to Analytical Chemistry, Wiley 1999.
• Kellner R., Mermet J.-M., Otto M., Widmer H. M., Analytical Chemistry, Wiley 1998.

Assessment methods (in Czech)

2 hodinová přednáška
kombinovaná zkouška (písemná a ústní část)

Language of instruction

Czech

Follow-Up Courses

• C4050 Analytical Chemistry II

Further Comments

The course can also be completed outside the examination period.
The course is taught annually.
The course is taught: every week.

Listed among pre-requisites of other courses

• C1660 Basic Analytical Chemistry
  !C3100 && !C4050 && !C5230 && !NOWANY(C3100,C4050,C5230)  
• C3110 Analytical Chemistry I - seminar
  NOW(C3100)  
• C3120 Analytical Chemistry - laboratory course
  (C1100||C4221) && (C3100||C1660)  
• C4050 Analytical Chemistry II
  C3100 && C3110  
• C5230 Analytical Chemistry
  !C3100 && !C4050 && !NOWANY(C3100,C4050)  
• C6160 Analytical chemistry II - seminar
  C3100 && C3110  

• Enrolment Statistics (recent)