Solubility of AgCN is maximum in :

Options

A. acidic buffer solution
B. basic buffer solution
C. in pure water
D. equal in all solution

Answer

To determine the maximum solubility of AgCN, we need to analyze how its solubility is affected by the presence of different ions in solution. Here’s a step-by-step breakdown of the solution:

### Step 1: Understand the Dissociation of AgCN
AgCN (Silver cyanide) dissociates in water to form Ag⁺ (silver ions) and CN⁻ (cyanide ions):
\[ \text{AgCN} \rightleftharpoons \text{Ag}^+ + \text{CN}^- \]

### Step 2: Consider the Effect of an Acidic Buffer
An acidic buffer contains a weak acid (HA) and its conjugate base (A⁻). When an acidic buffer is added to the solution, it increases the concentration of H⁺ ions:
\[ \text{HA} \rightleftharpoons \text{H}^+ + \text{A}^- \]

### Step 3: Reaction of H⁺ with CN⁻
The H⁺ ions from the acidic buffer will react with the CN⁻ ions to form HCN (hydrogen cyanide), which is a weak acid:
\[ \text{H}^+ + \text{CN}^- \rightleftharpoons \text{HCN} \]

### Step 4: Le Chatelier's Principle
According to Le Chatelier's principle, if the concentration of one of the products (in this case, CN⁻) is decreased (due to its reaction with H⁺), the equilibrium will shift to the left to produce more CN⁻ ions. This means that the dissociation of AgCN will be favored to replace the CN⁻ ions that are being consumed:
\[ \text{AgCN} \rightleftharpoons \text{Ag}^+ + \text{CN}^- \]

### Step 5: Conclusion on Solubility
Since the reaction shifts to the right to produce more CN⁻ ions, the solubility of AgCN will increase in an acidic buffer solution compared to pure water, where no such reaction occurs.

### Final Answer
The solubility of AgCN is maximum in an **acidic buffer solution**.

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