COURSE OBJECTIVE: To acquaint students with the analytical and critical approach to chemical analysis by applying knowledge about chemical equilibrium in order to qualify or quantify analyte and obtain useful information.
COURSE IMPLEMENTATION PROGRAM:
Lectures and seminars:
Week 1:
Introduction to the basics of chemical analysis and analytical chemistry. Sample-analyte-matrix-signal-information. Qualitative and quantitative information. Micro and macro concentrations of analytes. Limit of detection.
Week 2:
Chemical equilibrium in predicting analytical reactions for the determination and separation of analytes in various sample matrices.
Week 3:
Protolytic (acid-base) reactions. The role of acids and bases in analytical systems.
Week 4:
Polyprotic acids. Salt hydrolysis. Buffer systems.
Week 5:
Reactions of chemical complexes. Predicting ligand exchange reactions due to changes in medium conditions. Masking interferences by converting them into stable chemical complexes. Analytically important complexes.
Week 6:
Redox systems. Stability of different forms of analytes in aqueous media depending on pH. Selective oxidation and reduction of analytes.
Week 7:
First partial test. Equilibria in heterogeneous systems. Basic principles of precipitation reactions depending on pH, ligand, excess reagent, and foreign ions.
Week 8:
Principles and conditions of the dissolution process: dissolution by conversion into a weak electrolyte, by conversion into a chemical complex, and by electron exchange.
Week 9:
Solubility diagrams of sulfides, hydroxides, and carbonates. Amphotericity of precipitates.
Week 10:
Dissolution of a solid inorganic sample.
Week 11:
Selective dissolution and precipitation of chlorides and sulfides ? elimination of interferences. Systematic analysis of cations from groups I and II.
Week 12:
Selective dissolution and precipitation of hydroxides and carbonates. Systematic analysis of cations from groups III to VI.
Week 13:
Systematic analysis of anions.
Week 14:
Fundamentals of chromatography. The role of chromatography in qualitative analysis. Thin-layer chromatography.
Week 15:
Second partial test.
Laboratory practice:
1. Analysis of chlorides and sulfides in acidic medium
2. Analysis of hydroxides and sulfides in alkaline medium
3. Analysis of alkali and alkaline earth salts
4. Analysis of water-soluble salts
5. Analysis of water-insoluble salts
6. Determination of phenolic compounds by thin layer chromatography
7. Rapid tests for ion analysis in drinking water
DEVELOPMENT OF GENERAL AND SPECIFIC COMPETENCIES OF STUDENTS:
The student acquires basic knowledge for independent work in an analytical laboratory, an appropriate approach to chemical sample analysis, the ability to draw critical conclusions based on acquired knowledge and information on chemical changes obtained during experimental work, and the ability to write laboratory reports correctly in accordance with good laboratory practice.
STUDENT OBLIGATIONS IN TEACHING AND METHOD OF FULFILLMENT:
Regular attendance at lectures and seminars, Partial tests, Laboratory practice.
CONDITIONS FOR OBTAINING A SIGNATURE:
Successful completion of laboratory practice and regular attendance at lectures and seminars.
METHOD OF TEACHING:
Lectures, computational exercises (seminars), and experimental work in the laboratory.
METHOD OF ASSESSMENT OF KNOWLEDGE AND EXAM:
Two partial tests during the semester. Students may be exempt from the exam if they collect sufficient points from partial tests, laboratory exercises, and discussions. Otherwise, students must complete both the written and oral parts of the exam.
METHODS OF MONITORING THE QUALITY AND SUCCESS OF THE COURSE:
Student survey.
COURSE LEARNING OUTCOMES:
1. Distinguish analyte, analytical signal and information
2. Analyze the basic principles of the approach to chemical analysis
3. Comment on the equilibria of chemical reactions, the law of mass action and the principle according to Le Chatelier
4. Solve the problem of separation and detection of analytes from a complex sample by applying the principles of chemical equilibria
5. Distinguish heterogeneous from homogeneous chemical systems
6. Predict the behavior of the analytical system with respect to chemical equilibrium and changing conditions in the system
7. Link the acquired knowledge during the implementation of laboratory exercises
LEARNING OUTCOMES AT PROGRAM LEVEL:
1. solve qualitative and quantitative problems by applying appropriate chemical principles and theories
2. interpret chemical information and data
3. apply standard laboratory procedures and instrumentation for preparative or analytical purposes, for organic and inorganic systems
4. interpret the results of laboratory observations and measurements, their significance and connection with the relevant theory
5. assess the risks associated with using certain chemical substances or laboratory procedures.
TEACHING UNITS WITH ASSOCIATED LEARNING OUTCOMES AND EVALUATION CRITERIA:
Teaching unit
1. Introduction to analytical chemical analysis: from sample, through analytical signal, to information; limit of detection of analytes in a sample; chemical equilibrium and chemical reactions.
Learning outcomes
- Define analyte, analytical signal, and information
- Understand the basic principles underlying chemical analysis
Evaluation criteria
- Apply the basic principles of chemical analysis to identify and detect analytes
Teaching unit
2. Protolytic, complexometric, electrochemical, and precipitation reactions.
Learning outcomes
- Define equilibrium constants of chemical reactions, the law of mass action, and Le Chatelier's principle
- Apply the principles of chemical equilibrium to identify and separate analytes from a complex sample
Evaluation criteria
- Write chemical reactions and chemical equilibria
- Solve calculation problems using the law of mass action and Le Chatelier's principle
- Calculate the pH of buffer, amphoteric, acidic, and basic solutions
- Know the stability of complex compounds and spontaneous redox reactions
- Calculate the solubility product constant
Teaching unit
3. Reactions in homogeneous and heterogeneous systems; complex samples.
Learning outcomes
- Distinguish between heterogeneous and homogeneous chemical equilibrium systems
- Predict the behavior of a chemical reaction with changes in pH and the effects of common and foreign ions
Evaluation criteria
- Identify the analyte using acid-base reactions, reactions of chemical complexes, redox, and precipitation reactions
Teaching unit
4. Laboratory exercises
Learning outcomes
- Apply the principles of chemical equilibrium to identify and separate analytes from a complex sample
- Apply acquired knowledge as part of good laboratory practice when writing laboratory reports
Evaluation criteria
- Demonstrate knowledge and understanding of systematic analysis of cations and anions based on selective precipitation and dissolution of precipitates
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1. Š. Cerjan-Stefanović, Osnove analitičke kemije, Tehnološki fakultet, Zagreb, 1983.
2. Z. Šoljić, Kvalitativna kemijska analiza anorganskih tvari, FKIT, Zagreb, 2003.
3. Z. Šoljić, Računanje u kvantitativnoj kemijskoj analizi, Sveučilište u Zagrebu, Zagreb 1998.,
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1. G. Charlot, Les methodes de la chimie analytique, Masson et Cie, Paris, 1990.
2. D.C. Harris, Quantitative Chemical Analysis, W.H. Freedman and Co., New York, 2001.
3. M. Kaštelan-Macan, Kemijska analiza u sustavu kvalitete, Školska knjiga, Zagreb, 2003.
4. D.A. Skoog, D.M. West, F.J. Holler, Osnove analitičke kemije, 1. izd., Školska knjiga, Zagreb, 1999.,
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