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 by Barkeley –Hartley’s method; Elevation of boiling point and its measurement by Landsberger’s method ; Depression of freezing point and its measurement by Rast method ; Use of colligative properties in molecular weight determination; Non-ideal behaviour and Van’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.
Phase equilibria of two component system-solid-liquid equilibria , simple eutectic – Bi-Cd , Pb-Ag systems, desilverisation of lead.
Solid solutions: compound formation with congruent melting point (Mg-Zn) and incongruent melting point (NaCl-H2O), (FeCl3 – H2O) and (CuSO4 – H2O) system; freezing mixtures (acetone – dry ice).
Phase diagrams for three component systems.
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