Chemistry 11

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8.1.2 Law of Mass Action 8.1.2.1 Units of Equilibrium Constants

8.1.3 Equilibrium Constant Expressions for Some Important Reactions 8.1.3.2 ii. Dissociation of PCl5 (gaseous phase reaction)8.1.3.3 iii. Decomposition of N2O4 (gaseous phase reaction)8.1.3.4 iv. Synthesis of NH3 ( gaseous phase reaction)


8.1.5 Applications of Equilibrium Constant 8.1.5.1 (i) Direction of Reaction8.1.5.2 (ii) Extent of Reaction8.1.5.3 (iii) The Effect of Conditions on the Position of Equilibrium

8.1.6 The Le-Chateliers Principle 8.1.6.1 (a) Effect of Change in Concentration8.1.6.2 (b) Effect of Change in Pressure or Volume8.1.6.3 (c) Quantitative Effect of Volume on Equilibrium Position8.1.6.4 (d) Effect of Change in Temperature8.1.6.5 (e) Effect of Catalyst on Equilibrium Constant

8.2 Applications of Chemical Equilibrium in Industry 8.2.1 Synthesis of Ammonia by Haber?s Process8.2.2 Preparation of Sulphur Trioxide

8.3.0 IONIC PRODUCT OF WATER 8.3.1 pH and pOH

8.4.0 IONIZATION CONSTANTS OF ACIDS (Ka) 8.4.1 Percentage of Ionization of Acids

8.5.0 IONIZATION CONSTANT OF BASES (Kb) 8.5.1 pKa and pKb


8.7 COMMON ION EFFECT 8.7.1 More Examples of Common Ion Effect

8.8.0 Buffer Solutions 8.8.0.1 (a) Why Do We Need Buffer Solution?8.8.0.2 (b) How Do the Buffers Act?8.8.0.3 Calculating the pH of a Buffer8.8.1 Buffer Capacity

8.9.0 EQUILIBRIA OF SLIGHTLY SOLUBLE IONIC COMPOUNDS (SOLUBILITY PRODUCT) 8.9.1 Applications of solubility product8.9.1.1 (a) Determination of Ksp, from solubility8.9.1.2 (b) Determination of Solubility from Ksp