Assertion (A): Solubility of `AgCN` in acidic solutions is greater than in pure water.
Reason (R) : Solubility equilibrium of `AgCN` is shifted in forward direction due to the formation of `HCN`.

Options

A. If both the statements are TRUE and STATEMENT-2 is the correct explation of STATEMENT-1
B. If both the statements are TRUE AND STATEMENT-2 is NOT the correct explanation of STATEMENT-1
C. If STATEMENT-1 is TRUE and STATEMETN-2 is FLASE
D. If STATEMENT-1 is FLASE and STATEMENT-2 is TRUE

Answer

To solve the question regarding the assertion and reason about the solubility of AgCN in acidic solutions, we can break it down into the following steps:

### Step 1: Understand the Assertion
The assertion states that the solubility of AgCN in acidic solutions is greater than in pure water.

**Hint:** Consider how the presence of acid might affect the solubility of a salt.

### Step 2: Analyze the Solubility of AgCN
AgCN (silver cyanide) dissociates in water as follows:
\[ \text{AgCN (s)} \rightleftharpoons \text{Ag}^+ (aq) + \text{CN}^- (aq) \]

In pure water, this equilibrium exists, and both Ag⁺ and CN⁻ ions are present.

**Hint:** Think about what happens to the ions in the solution when you introduce an acid.

### Step 3: Consider the Effect of Acid
In an acidic solution, the concentration of H⁺ ions increases. The CN⁻ ions can react with H⁺ ions to form HCN (hydrogen cyanide):
\[ \text{CN}^- (aq) + \text{H}^+ (aq) \rightarrow \text{HCN} (aq) \]

This reaction will decrease the concentration of CN⁻ ions in the solution.

**Hint:** Recall Le Chatelier's principle, which states that if a system at equilibrium is disturbed, the system will shift in a direction that counteracts the disturbance.

### Step 4: Apply Le Chatelier's Principle
Since the concentration of CN⁻ decreases due to its reaction with H⁺ ions, the equilibrium of the dissociation of AgCN will shift to the right (forward direction) to produce more CN⁻ ions:
\[ \text{AgCN (s)} \rightleftharpoons \text{Ag}^+ (aq) + \text{CN}^- (aq) \]

This shift increases the solubility of AgCN in the acidic solution.

**Hint:** Think about how the equilibrium shift affects the overall concentration of ions in the solution.

### Step 5: Conclusion
Both the assertion and reason are correct:
- The solubility of AgCN in acidic solutions is indeed greater than in pure water.
- The reason provided (formation of HCN) correctly explains why the solubility increases due to the shift in equilibrium.

### Final Answer
Both the assertion and reason are true, and the reason is the correct explanation for the assertion.