Exercises in General Chemistry

Code

Course teacher

Associate teachers

Status of the course

Course objectives

Exercising, testing and confirm knowledge from lectures. Understanding with the methods of experimental work and the acquisition of skills necessary for independent work in the lab.

Course enrolment requirements and entry competences required for the course

Enrolled in or passed the course General Chemistry

Learning outcomes expected at the level of the course (4 to 10 learning outcomes)

Students will upon completion of the course be able to:
1. Practically through experiments verify the theoretical assumptions
2. Gain independence in performing experiments
3. Design simple experiments to illustrate the chemical properties of the substance
4. Actively exploring ways in which this discipline has consequently impact on the outside world.

Course content broken down in detail by weekly class schedule (syllabus)

Exercise 1
The basic rules of laboratory work, safety precautions and protection in the lab, basic laboratory equipment. Washing, cleaning and drying of dishes. Basic laboratory operations, chemicals and dealing with them. Decomposition of the substance to the pure substance. Decomposition of heterogeneous and homogeneous mixture
Exercise 2
Decomposition of the mixture to the pure substance, Decomposition of heterogeneous substances, Sedimentation, decanting, centrifuging, filtering, Buchner funnel, distillation and fractional distillation, sublimation of iodine. Extraction of iodine from aqueous solutions
Exercise 3
Physical and chemical changes, the law of conservation of weight, Gay - Lussac’s law of connected volumes. Exercise with models of unit cells. Determining the relative atomic mass of zinc. Determination of the empirical formula of copper chloride.
Exercise 4
Gas Laws: Determination of the molar volume of oxygen, Boyle’s law, Charles Gay - Lussac’s law, the pressure dependence of the temperature in gases.
Exercise 5
Solutions and their properties. Expressing of concentration. Preparation of the solution with given concentration. Solutions of liquids in liquids. Solutions of gases in liquids. Dependence of solubility on the nature (structure) of the substance. Dependence of solubility on temperature. Dissolution of liquids in liquids. Dissolving gases in liquids. Henry’s law. Determination of molar mass by freezing point depression. Illustration of electrolytic dissociation. Illustration of ions traveling to the electrodes. Electrical conductivity of the solution. Redox - reactions of sulfur and oxygen. Redox reaction of dilute nitric acid solution and iron (II) sulfate. Decomposition and formation reactions of complexes. Ligand substitution reaction. Protolytic reactions (acid- base titration).
Exercise 6
Chemical kinetic, effect of concentration of reactants on the rate of chemical reactions. Effect of temperature on the rate of chemical reactions. The catalytic effect on the rate of chemical reactions. Balance in electrolyte solutions. Moving the chemical balance. Determination of the acid dissociation constant, Ka . Determination of pH: Approximately determination of pH using indicators. Determination of pH using pH sensors. Electrolysis - Determination of Faraday’s constant. Electromotive force of galvanic cells - Daniell cell.
Exercise 7
Protolytic reactions and titration curves obtained with the help of computers
Determination of the acid dissociation constant, Ka. Hydrolysis. Buffers.
Exercise 8
Vacuum distillation. Determination of the molar mass of easily volatile liquids.
Determination of molar mass by freezing point depression

Format of instruction:

Student responsibilities

Completed all laboratory exercises.

Optional literature (at the time of submission of study programme proposal)

Quality assurance methods that ensure the acquisition of exit competences

- Information from interviews, observations, and consultation with students during lectures
- Student survey

Other (as the proposer wishes to add)