Chemistry Practice I. Laboratory

Short syllabus of the subject:

Expression for the composition of solutions and their applications. Operations with solutions, crystallization, recrystallization.

Gases. Properties of gases. Equation of state for ideal gas, and its versions. Boyle’s law, Charles’ laws. Gay-Lussac’ law.

Mixtures of gases, compositions. Partial pressure, and volume. Dalton’s rule and Amagat’s rule. Vapor pressure.

Colligative properties of dilute solutions. Vapor pressure lowering, boiling-point elevation, and freezing-point depression, osmosis.

Balancing equations. Oxidation numbers, redox equations.

Stoichiometry and its applications. Yield. Avogadro’s law. Calculation of titration.

Basic terms in thermochemistry. Energy, heat and enthalpy. Heat capacity, molar heat capacity.

The heat of reactions and Hess's law.

General description of chemical equilibria. Various forms of equilibrium constants and their connections.

Application of LeChatelier's principle. The shift in the equilibrium composition by the change in the amount of reactants, in the pressure, and in the temperature.

Acid-base equilibria, pH of solutions:

-          Strong acids and bases;

-          Weak acids and bases;

-          Hydrolysis of salts;

-          Buffers and buffer capacities

Solubility equilibria: solubility product and its applications, common ion effect; speciation effect; temperature effect.

Electrochemisty:

-          Electrolyte solutions. Electrical resistance and conductivity of dilute solutions;

-          Electrolysis;

-          Electrode potentials: standard hydrogen electrode, simple metal electrodes, redox electrodes

-          Composition dependence of electrode potentials in various electrode types: Nernst equation.

-          Electrochemical cells, cell diagrams, cell reactions, half-cell reactions. Electromotive force.

-          Basic terms in electrochemistry, direction of electrochemical processes.