Methods for equilibria constants determination in solutions 0600-S1-CM-PW7c-MWSR

The course consists of a lecture and a laboratory.
The lecture presents the theoretical basis for defining equilibrium constants encountered in the chemistry of solutions. It presents examples of such constants (for example protonation and complexation constants (taking into account the chemistry of enzymes), solubility products, and equilibria existing in two-phase solutions (incompatible solvents - partition coefficient)). In the further part of the lecture, the basic methods used to determine the presented constants will be presented (e.g. spectrophotometric, potentiometric, and conductometric methods, but also the use of fluorescence spectrometry, NMR and HPLC).
The laboratory is an illustration of the information presented in the lecture. Six experiments will be carried out within the experimental activities. Their implementation will allow for the determination of several different types of chemical equilibrium constants using various methods (UV-Vis, conductometry, acid-base, potentiometry).
The topics of the proposed laboratory classes are listed below:
1. Determination of the protonation constants of the selected amino acid or organic dye.
2. Dissolution equilibria of a selected inorganic salt (e.g. CaSO4‧2H2O). The influence of ionic strength.
3. Determining the activation energy and the equilibrium constant of the selected reaction (e.g. ferroin dissociation).
4. Influence of ligand coordination on its pKa value.
5. Determination of the partition coefficient (e.g. for sulphanilamide in the water-octanol system).
6. Determination of the equilibrium constant characterizing the step of the reversible reaction preceding the rate-limiting step of the process (Michaelis-Menten kinetics).

Total student workload

a. 15 h – lecture, i.e. 15 contact hours; b. 30 h – laboratory, i.e. 30 contact hours; c. 25 h – individual work, d. 30 h – time required for preparation in the assessment process. The total student workload is 100 h/25 = 4 ECTS.

Learning outcomes - knowledge

W1: Describes the basic concepts of equilibria existing in solutions - K_W01; W2: Characterizes the equilibrium processes observed in everyday life (complexation, acidification) - K_W09; W3: Knows the basic concepts in the field of solution chemistry, physical chemistry, including kinetics (equilibrium, limiting step, partition coefficient, etc.) - K_W10.

Learning outcomes - skills

U1: Can use chemical nomenclature and concepts in the field of physical chemistry and chemical kinetics - K_U01; U2: Can properly define equilibrium constants depending on the analyzed chemical reaction - K_U02; U3: Can find relations between the observed physicochemical changes in the system and the model that describes them - K_U13.

Learning outcomes - social competencies

K1: Works independently and effectively with a large amount of information, sees relationships between phenomena, and correctly draws conclusions using the principles of logic (analytical thinking) - K_K01; K2: Is focused on the continuous acquisition of new knowledge, skills, and experiences; sees the need for continuous improvement and improvement of professional competencies; knows the limitations of his own knowledge and understands the need for further education (striving for development) - K_K05; K3: Knows and observes the rules and standards applicable to a chemist, including ethical standards; understands the social role of the profession; understands and appreciates the importance of intellectual honesty, care for the health and the natural environment in the activities of their own and others (professionalism and ethics) - K_K08.

Teaching methods

Lecture: - Lecture combined with discussion; - Case study. Laboratory: - Laboratory method (participation in scheduled laboratory exercises); - Experimental method; - Problem method (discussion with pairs while carrying out a given task); - Research method (reports).

Expository teaching methods

- problem-based lecture
- informative (conventional) lecture
- participatory lecture
- narration

Exploratory teaching methods

- biographical
- laboratory
- presentation of a paper
- seminar
- practical
- classic problem-solving
- experimental

Prerequisites

Knowledge of general chemistry and mathematics.

Course coordinators

Adrian Topolski

Assessment criteria

Lecture (60%), Laboratory (40%).

The method of verification of learning outcomes:
Graded test of the lecture: W1, W2, W3
Laboratory report: K1, K2, K3, W1, W2, U1, U2, U3

Practical placement

Bibliography

1. Kędryna, T., Chemia ogólna z elementami biochemii, Wyd. "Zamiast korepetycji", Kraków 1994.
2. Kita E., Kita P., Ćwiczenia laboratoryjne z kinetyki chemicznej, Wyd. UMK w Toruniu, Toruń 1993.
3. Galus, Z., Ćwiczenia rachunkowe z chemii analitycznej, Wydawnictwa Naukowe PWN, Warszawa 1996.
4. Ufnalski W., Obliczenia fizykochemiczne, Oficyna Wydawnicza Politechniki Warszawskiej, Warszawa 1995.
5. Bielański, A., Podstawy chemii nieorganicznej, t.1, wyd. VI, Wydawnictwo Naukowe PWN, Warszawa 2010.

Additional information

Additional information (registration calendar, class conductors, localization and schedules of classes), might be available in the USOSweb system:

Description of 0600-S1-CM-PW7c-MWSR in USOSweb