IONIC EQUILIBRIUM
Numerical Solution
Learning Outcomes:
2. Ionic Equilibrium
2.1 Explain the limitations of Arrhenius concepts of acids and bases.
2.2 Define Bronsted and Lowry concepts for acids and bases.
2.3 Define conjugate acids and conjugate base.
2.4 Identify conjugate acid-base pairs of Bronsted acid and base.
2.5 Define and explain Lewis acids and bases.
2.6 Use the extent of ionization and dissociation constant of acid (ka) and base (kb).
2.7 Explain ionization constant of water and calculate pH and pOH in aqueous medium using Kw values.
2.8 Show understanding of, and use, the concept of solubility product Ksp.
2.9 Calculate Ksp from concentrations and vice versa.
2.10 Show understanding of the common ion effect.
2.11 Describe the application of solubility product principle and common ion effect in precipitation reactions.
2.12 Define a Buffer and show with equations how a Buffer system works.
2.13 Explain the choice of suitable indicators for acid-base titrations and describe the changes in pH during acid-base titrations.
2.14 Define and differentiate different types of salts (simple salts, double salts, complex salt, acidic salts, basic salts and neutral salts).
2.15 Explain hydrolysis of salts (salts of strong acid and strong base, salts of weak acid and strong base and salts of weak base and strong acid).
Syllabus:
2. Ionic Equilibrium
Introduction to Acids and Bases
2.1. Limitation of Arrhenius concepts of acids and bases
2.2 Bronsted –Lowry definition of acids and bases
2.3 Relative strength of acids and bases
2.4 Conjugate acid–base pairs
2.5 Lewis definition of acids and bases
2.6 Ionization of weak electrolyte (Ostwald's dilution law)
2.7 Ionic product of water(Kw)
2.8 Dissociation constant of acid and base, (Ka& Kb)
2.9 Concept of pKa and pKb
2.10 pH value: pH of strong and weak acids, pH of strong and weak bases
2.11 Solubility and solubility product principle
2.12 Common Ion effect
2.13 Application of solubility product principle and common ion effect in precipitation reactions
2.14 Buffer solution and its application
2.15 Indicators and selection of indicators in acid base titration
2.16 Types of salts: Acidic salts, basic salts, simple salts, complex salts (introduction and examples)
2.17 Hydrolysis of salts
2.17.1 Salts of strong acid and strong base
2.17.2 Salts of weak acid and strong base
2.17.3 Salts of weak base and strong acid
(solving related numerical problems)
