Strong, moderate and weak electrolytes, degree of ionization, factors affecting degree of ionization, ionization constant and ionic product of water. Ionization of weak acids and bases, pH scale, common ion effect; dissociation constants of mono-, di- and tri- protic acids (exact treatment). Salt hydrolysis-calculation of hydrolysis constant, degree of hydrolysis and pH for different salts. Buffer solutions; derivation of Henderson equation and its applications; Buffer capacity, buffer range, buffer action and applications of buffers in analytical chemistry and biochemical processes in the human body. Solubility and solubility product of sparingly soluble salts – applications of solubility product principle. Qualitative treatment of acid – base titration curves (calculation of pH at various stages). Theory of acid – base indicators; selection of indicators and their limitations. Multistage equilibria in polyelectrolyte systems; hydrolysis and hydrolysis constants.

Introduction, colligative properties, Raoult’s law, relative lowering of vapour pressure; Osmosis, law of osmotic pressure and its measurement, Elevation of boiling point and its measurement, Depression of freezing point and its measurement, Use of colligative properties in molecular weight determination; Non-ideal behaviourandvan’t Hoff’s factor ‘i’.

Solutions: Ideal and non-ideal solutions, methods of expressing concentrations of solutions, Solution of gases in liquid: Henry’s law, deviation from Henry’s law. Non ideal system: Azeotropes –ethanol-water systems. Partially miscible liquids: Phenol-water, trimethylamine-water, nicotine-water systems; lower and upper consolute temperature, effect of impurity on consolute temperature; Immiscible liquids.

Introduction to phase, component and degree of freedom, derivation of Gibbs phase rule; Phase equilibria of one component system-water, CO₂ and sulphur system, liquid helium.

Phase equilibria of two component system-solid-liquid equilibria, simple eutectic – Bi-Cd, KI-H₂O, Pb-Ag systems, desilverisation of lead.

Solid solutions: Compound formation with congruent melting point (Mg-Zn) and incongruent melting point (NaCl-H₂O), (FeCl₃ – H₂O), (CuSO₄ – H₂O) and (Na₂SO₄–H₂O) system; freezing mixtures (acetone – dry ice).

Phase diagrams for three component systems. Acetic acid –chloroform-water.