1. Consider the hydrolysis of ammonium acetate
CH3COONH4(aq) → CH3COO- (aq) + NH4+(aq)
2. In this case both the cation (NH4+) and (CH3COO-) anion have the tendency to react with water.
CH3COO- +H2O ⇌ CH3COOH + OH-
NH4 + H2O ⇌ NH4OH + H3
3. The nature of the solution depends on the strength of acid (or) base i.e., if Ka > Kb , then the solution is acidic and pH < 7, if Ka < Kb then the solution is basic and pH > 7. If Ka = Kb , then the solution is neutral.
4. The relation between the dissociation constant Ka , Kb and hydrolysis constant is given by the following expression.
Ka . Kb . Kh = Kw
5. pH of the solution
pH = 7 + \(\frac{1}{2}pK_a-\frac{1}{2}pK_b\)