Hydrolysis is an acid-basedreaction of a cation or anion or both ions of a salt with water, Resultan solution of hydrolysis may be acidic, basic or netural. The anion `A^(-)` which is a weakeer base than `OH^(-)` and which his its conjugate acid HA stronger then water but weaker than `H_(3)O` shown the phenomenon of hydrolysis Ex : `CH_(3)COO^(-),CN^(-),NO_(2)^(-)` etc.
The contion `B^(+)` which is a weaker acid than `H_(3)^(+)` which is a weaker acid then `H_(3)^(+)` and which has its conjugate base BOH stronger than water but weak than `OH^(-)` shown the phenmenon of hydrolysis Ex : `NH_(4)^(+)C_(6)H_(5)NH^(+),N_(2)H_(5)^(+)` etc.
The hydrolysis constant of anion and cation are given by
`A^(-)(aq.)+H_(2)O(l)hArrHA(aq.)+OH^(-)(aq)`
`" " K_(h)=(K_(w))/(K_(a))rArr([HA(aq.)][OH^(-)(aq.)])/([A^(-)(aq.)])`
`B^(+)(aq.)+H_(2)O(l)hArrBOH(aq.)+H^(+)(aq.)`
`" " K_(h)=(K_(w))/(K_(b))rArr([BOH(aq.)][H^(+)(aq.)])/([B^(-)(aq.)])`
Which of the following statement is true

Options

A. Weaker the acid, greater statement is true?
B. Weaker the base, greater will be hydrolysis of its anion
C. Both (a) and (b)
D. None of these

Answer

To solve the question regarding hydrolysis and the statements provided, we will analyze the concepts of hydrolysis constants for anions and cations, and then evaluate the truth of the statements.

### Step-by-Step Solution:

1. **Understanding Hydrolysis**: Hydrolysis is the reaction of a salt with water, leading to the formation of an acid and a base. The resulting solution can be acidic, basic, or neutral depending on the nature of the ions involved.

2. **Analyzing the Anion Hydrolysis**:
- For an anion \( A^- \) that is a weaker base than \( OH^- \), the hydrolysis reaction can be represented as:
\[ A^-(aq) + H_2O(l) \rightleftharpoons HA(aq) + OH^-(aq) \]
- The hydrolysis constant \( K_h \) for this reaction is given by:
\[ K_h = \frac{K_w}{K_a} \]
- Here, \( K_w \) is the ion product of water, and \( K_a \) is the acid dissociation constant of the conjugate acid \( HA \). A weaker base \( A^- \) will have a larger \( K_a \), leading to a smaller \( K_h \).

3. **Analyzing the Cation Hydrolysis**:
- For a cation \( B^+ \) that is a weaker acid than \( H_3O^+ \), the hydrolysis reaction can be represented as:
\[ B^+(aq) + H_2O(l) \rightleftharpoons BOH(aq) + H^+(aq) \]
- The hydrolysis constant \( K_h \) for this reaction is given by:
\[ K_h = \frac{K_w}{K_b} \]
- Here, \( K_b \) is the base dissociation constant of the conjugate base \( BOH \). A weaker acid \( B^+ \) will have a larger \( K_b \), leading to a smaller \( K_h \).

4. **Evaluating the Statements**:
- **Statement 1**: "Weaker the acid, greater will be the hydrolysis of its cation."
- This statement is **false** because a weaker acid results in a smaller hydrolysis constant, leading to less hydrolysis.

- **Statement 2**: "Weaker the base, greater will be the hydrolysis of its anion."
- This statement is also **false** because a weaker base results in a smaller hydrolysis constant, leading to less hydrolysis.

5. **Conclusion**: Since both statements are false, the answer to the question is that **none of the statements are true**.