Contents

1. Ionic Equilibria

1. pH

2. Buffer

2.1 Action of Buffer Solution

2.2 Mass Law Equation

2.3 Derivation of the Equation

3. Equilibrium Constants

4. Relationship between kc and kp

4.1 Significance of the Magnitude of Equilibrium Constant

4.2 Characteristics of Equilibrium Constant

4.3 Le-Chatelier’s Principle

4.4 Classical Definitions of Acids and Bases

4.5 Arrhenius Theory of Acids and Bases

4.6 Lowry Bronsted Concept

4.7 Conjugate Acid Base Pair

4.8 Amphoteric Nature of Water

4.9 Lewis Concept of Acids and Bases

5. Strong and Weak Acids and Bases

5.1 Degree of Dissociation (?)

5.2 Strength of Acid

5.3 Strength of Base

5.4 Ostwald’s Dilution Law

6. Ionisation of Water

7. Acid Base Titrations

7.1 Neutralization Curves

7.2 Henderson Hasselbalch Equation

8. Solubility Product

8.1 Technical Applications of Solubility Product

8.2 Applications to Analytical Chemistry

8.3 Examples

9. Osmosis

9.1 Osmotic Pressure

2. Chemical Kinetics

1. Introduction

1.1 Types of Reactions

1.2 Rate of Reactions or Reaction Velocity

1.3 Factors Affecting Rate of Reaction or Reaction Velocity

1.4 Law of Mass Action and Rate Law

1.5 Rate Constant and its Significance

2. Molecularity and Order

2.1 Molecularity of Reaction

2.2 Order of Reaction

3. Experimental Methods to Study Rate of Chemical Reactions

4. Terminology of Chemical Kinetics

5. Zero Order Reaction

6. First Order Reaction

6.1 Characteristic of First Order Reaction

6.2 Examples of First order Reactions

7. Second Order Reaction

7.1 Characteristics of Second Order Reaction

7.2 Examples of Second Order Reaction

8. Third Order Reaction

8.1 Characteristics of Third Order Reaction

8.2 Examples of Third Order Reactions

9. Pseudo Molecular Reaction

10. Effect of Temperature on Rate of Reaction

10.1 Derivation of Arrhenius Equation

10.2 Determination of Energy of Activation

11. The Energy of Activation

3. Electrochemistry

1. Introduction

2. Reversible and Irreversible Cells

2.1 Reversible Cells

2.2 Irreversible Cells

3. Electromotive Force (E.M.F.)

3.1 Origin of E.M.F. (Nernst 1889)

3.2 Measurement of E.M.F. (Electromotive Force)

4. Standard Cell

4.1 Cell Reaction and E.M.F.

4.2 Convention Regarding Sign of E.M.F.

5. Single Electrode Potential

5.1 Reference Electrodes

5.2 Determination of Single Electrode Potential

6. Calculation of Cell e.m.f

6.1 Oxidation Potential, Reduction Potential and Electrodes Potential

6.2 Determination of ECell

6.3 Summary of Rules

7. Thermodynamics and E.M.F

8. Liquid Junction Potential

9. Debye-Huckel-Onsagar Equation

10. Over Voltage/Over Potential

4. Basics of Mole Concept

1. Relationship between Molecular Weight and Vapour Density

1.1 Absolute Density

2. Molar Volume or Gram Molecular Volume (GMV)

3. Avogadro’s Number

4. Mole Concept

5. Relationship between Molecular Weight and Vapour Density

5.1 Absolute Density

6. Molecular Weight

7. Modes of Expressing Composition (Concentration) of Solution

8. Ideal Dilute Solution

9. Raoult’s Law