› 6.1.1 Solid-Liquid Equilibrium
› 6.1.2 Liquid-Vapour Equilibrium
› 6.1.3 Solid – Vapour Equilibrium
› 6.1.4 Equilibrium Involving Dissolution
› 6.1.5 General Characteristics of
› 6.4 Homogeneous Equilibria
› 6.4.1 Equilibrium Constant in Gaseous Systems
› 6.5 Heterogeneous Equilibria
› 6.6.1 Predicting the Extent of a
› 6.6.2 Predicting the Direction of the Reaction
› 6.6.3 Calculating Equilibrium
› 6.8.1 Effect of Concentration Change
› 6.8.2 Effect of Pressure Change
› 6.8.3 Effect of Inert Gas Addition
› 6.8.4 Effect of Temperature Change
› 6.8.5 Effect of a Catalyst
› 6.9 Ionic Equilibrium in Solution
› 6.10 Acids, Bases and Salts
› 6.10.1 Arrhenius Concept of Acids and Bases
› 6.10.2 The Brönsted-Lowry Acids and Bases
› 6.10.3 Lewis Acids and Bases
› 6.11 Ionization of Acids and Bases
› 6.11.1 The Ionization Constant of Water
› 6.11.2 The pH Scale
› 6.11.3 Ionization Constants of Weak Acids
› 6.11.5 Relation between Ka and Kb
› 6.11.6 Di- and Polybasic Acids and Di-
› 6.11.8 Common Ion Effect in the
› 6.11.7 Factors Affecting Acid Strength
› 6.11.9 Hydrolysis of Salts and the pH of their Solutions
› 6.12 Buffer Solutions
› 6.12.1 Designing Buffer Solution
› 6.13 Solubility Equilibria of
› 6.13.1 Solubility Product Constant
› 6.13.2 Common Ion Effect on Solubility