dissociation, combustion, formation, atomization, sublimation, phase transition, hydration,
ionization, and solution.
The second law of thermodynamics - Spontaneity of processes; S of the universe and G
of the system as criteria for spontaneity. G (Standard Gibbs energy change) and equilibrium
constant.
UNIT 5: SOLUTIONS
Different methods for expressing the concentration of solution - molality, molarity, mole
fraction, percentage (by volume and mass both), the vapour pressure of solutions and Raoult's
Law - Ideal and non-ideal solutions, vapour pressure - composition, plots for ideal and non-
ideal solutions; Colligative properties of dilute solutions - a relative lowering of vapour
pressure, depression of freezing point, the elevation of boiling point and osmotic pressure;
Determination of molecular mass using colligative properties; Abnormal value of molar mass,
van’t Hoff factor and its significance.
UNIT 6: EQUILIBRIUM
Meaning of equilibrium is the concept of dynamic equilibrium.
Equilibria involving physical processes: Solid-liquid, liquid-gas - gas and solid-gas
equilibria, Henry's law. General characteristics of equilibrium involving physical processes.
Equilibrium involving chemical processes: Law of chemical equilibrium, equilibrium
constants (K
p
and K
c
) and their significance, the significance of G and G in chemical
equilibrium, factors affecting equilibrium concentration, pressure, temperature, the effect of
catalyst; Le Chatelier’s principle.
Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts
of acids and bases (Arrhenius. Bronsted - Lowry and Lewis) and their ionization, acid-base
equilibria (including multistage ionization) and ionization constants, ionization of water. pH
scale, common ion effect, hydrolysis of salts and pH of their solutions, the solubility of
sparingly soluble salts and solubility products, and buffer solutions.
UNIT 7: REDOX REACTIONS AND ELECTROCHEMISTRY
Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for
assigning oxidation number, and balancing of redox reactions.
Electrolytic and metallic conduction, conductance in electrolytic solutions, molar
conductivities and their variation with concentration: Kohlrausch’s law and its applications.
Electrochemical cells - Electrolytic and Galvanic cells, different types of electrodes, electrode
potentials including standard electrode potential, half-cell and cell reactions, emf of a Galvanic
cell and its measurement: Nernst equation and its applications; Relationship between cell
potential and Gibbs' energy change: Dry cell and lead accumulator; Fuel cells.
UNIT 8: CHEMICAL KINETICS
Rate of a chemical reaction, factors affecting the rate of reactions: concentration, temperature,
pressure, and catalyst; elementary and complex reactions, order and molecularity of reactions,
rate law, rate constant and its units, differential and integral forms of zero and first-order