The solubility of AgCl will be minimum in

Options

A. `0.1 M CaCl_2`
B. `0.01 M AgNO_3`
C. Pure water
D. `0.1 M NH_3`

Answer

To determine the minimum solubility of AgCl, we need to consider the common ion effect and the presence of other ions in the solution that can affect the solubility of AgCl.

### Step-by-Step Solution:

1. **Understanding the Dissolution of AgCl**:
- AgCl dissociates in water according to the equation:
\[ \text{AgCl (s)} \rightleftharpoons \text{Ag}^+ (aq) + \text{Cl}^- (aq) \]

2. **Identifying the Common Ion Effect**:
- The solubility of a salt is reduced in the presence of a common ion. In this case, both Ag\(^+\) and Cl\(^-\) ions can act as common ions.

3. **Adding a Salt with Common Ions**:
- If we add a salt that contains either Ag\(^+\) or Cl\(^-\), it will shift the equilibrium to the left according to Le Chatelier's principle, thus reducing the solubility of AgCl.

4. **Considering Different Scenarios**:
- If we add NaCl (which provides Cl\(^-\)), the concentration of Cl\(^-\) increases, leading to a decrease in the solubility of AgCl.
- If we add AgNO\(_3\) (which provides Ag\(^+\)), the concentration of Ag\(^+\) increases, also leading to a decrease in the solubility of AgCl.

5. **Conclusion**:
- The solubility of AgCl will be minimum in a solution where there is a high concentration of either Ag\(^+\) or Cl\(^-\) ions. Therefore, adding a salt like NaCl or AgNO\(_3\) will significantly reduce the solubility of AgCl.

6. **Final Answer**:
- The solubility of AgCl will be minimum in a solution containing a common ion, such as NaCl or AgNO\(_3\).