Silver chloride is more soluble in very concentrated sodium chloride solution than in pure water. (T/F)

Explanation

To determine whether silver chloride (AgCl) is more soluble in very concentrated sodium chloride (NaCl) solution than in pure water, we can analyze the situation step by step.

### Step-by-Step Solution:

1. **Understanding Silver Chloride Solubility**:
- Silver chloride (AgCl) is a sparingly soluble salt. In pure water, when AgCl is added, it dissociates into silver ions (Ag⁺) and chloride ions (Cl⁻):
\[ \text{AgCl (s)} \rightleftharpoons \text{Ag}^+ (aq) + \text{Cl}^- (aq) \]

2. **Dissociation of Sodium Chloride**:
- Sodium chloride (NaCl) is a strong electrolyte, meaning it completely dissociates in solution into sodium ions (Na⁺) and chloride ions (Cl⁻):
\[ \text{NaCl (s)} \rightarrow \text{Na}^+ (aq) + \text{Cl}^- (aq) \]

3. **Effect of Concentrated Sodium Chloride Solution**:
- In a very concentrated NaCl solution, the concentration of Cl⁻ ions is significantly higher than in pure water. This introduces a common ion (Cl⁻) into the solution.

4. **Common Ion Effect**:
- The presence of a common ion (Cl⁻ from NaCl) affects the solubility of AgCl. According to Le Chatelier's principle, adding more Cl⁻ ions will shift the equilibrium of the dissociation of AgCl to the left:
\[ \text{Ag}^+ (aq) + \text{Cl}^- (aq) \rightleftharpoons \text{AgCl (s)} \]
- This means that more AgCl will precipitate out of the solution, reducing the amount of Ag⁺ and Cl⁻ ions in the solution.

5. **Conclusion**:
- Therefore, the solubility of AgCl decreases in very concentrated NaCl solution due to the common ion effect. This means that AgCl is **not** more soluble in concentrated NaCl than in pure water.

### Final Answer:
The statement "Silver chloride is more soluble in very concentrated sodium chloride solution than in pure water" is **False**.