Chemistry Grade 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 PCl<sub>5</sub> (gaseous phase reaction) 8.1.3.3 iii. Decomposition of N<sub>2</sub>O<sub>4</sub> (gaseous phase reaction) 8.1.3.4 iv. Synthesis of NH<sub>3</sub> ( gaseous phase reaction)

8.1.5 Applications of Equilibrium Constant 8.1.5.1 (i) Direction of Reaction 8.1.5.2 (ii) Extent of Reaction 8.1.5.3 (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 Concentration 8.1.6.2 (b) Effect of Change in Pressure or Volume 8.1.6.3 (c) Quantitative Effect of Volume on Equilibrium Position 8.1.6.4 (d) Effect of Change in Temperature 8.1.6.5 (e) Effect of Catalyst on Equilibrium Constant
8.2 Applications of Chemical Equilibrium in Industry 8.2.1 Synthesis of Ammonia by Haber`s Process 8.2.2 Preparation of Sulphur Trioxide
8.3.0 IONIC PRODUCT OF WATER 8.3.1 pH and pOH
8.4.0 IONIZATION CONSTANTS OF ACIDS (K<sub>a</sub>) 8.4.1 Percentage of Ionization of Acids
8.5.0 IONIZATION CONSTANT OF BASES (K<sub>b</sub>) 8.5.1 pK<sub>a</sub> and pK<sub>b</sub>

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 Buffer 8.8.1 Buffer Capacity
8.9.0 EQUILIBRIA OF SLIGHTLY SOLUBLE IONIC COMPOUNDS (SOLUBILITY PRODUCT) 8.9.1 Applications of solubility product 8.9.1.1 (a) Determination of K<sub>sp</sub>, from solubility 8.9.1.2 (b) Determination of Solubility from K<sub>sp</sub>