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Discuss about the hydrolysis of salt of weak acid and weak base and derive pH value for the solution.

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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 + \(\frac{1}{2}pK_a-\frac{1}{2}pK_b\)

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