`H_(2)S` will precipitate the sulphide of all the metals from the solution of chlorides of `Cu,Zn and Cd` if

Options

A. The solution is aqueous
B. The solution is acidic
C. The solution is diute acidic
D. Any of the above solution is present

Explanation

To solve the question regarding the precipitation of sulfides from the chlorides of copper (Cu), zinc (Zn), and cadmium (Cd) using hydrogen sulfide (H₂S), we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Reaction**:
- Hydrogen sulfide (H₂S) can react with metal ions to form metal sulfides. The general reaction can be represented as:
\[ \text{M}^{2+} + \text{H}_2\text{S} \rightarrow \text{MS} + 2\text{H}^+ \]
- Here, M represents the metal ions (Cu²⁺, Zn²⁺, Cd²⁺).

2. **Identifying the Conditions for Precipitation**:
- For H₂S to effectively precipitate the sulfides of the metals, the solution must provide sufficient sulfide ions (S²⁻).
- This occurs in an aqueous solution where H₂S can dissociate to provide sulfide ions.

3. **Analyzing the pH of the Solution**:
- In an **acidic solution**, H₂S remains largely undissociated, which means there are fewer sulfide ions available to precipitate the metal sulfides.
- In a **neutral or slightly basic solution**, H₂S can dissociate more effectively, providing the necessary sulfide ions.

4. **Conclusion**:
- Therefore, H₂S will precipitate the sulfides of copper, zinc, and cadmium if the solution is **aqueous** (neutral or slightly basic).
- The correct answer to the question is that H₂S will precipitate the sulfides if the solution is **aqueous**.

### Final Answer:
H₂S will precipitate the sulfide of all the metals from the solution of chlorides of Cu, Zn, and Cd if the solution is **aqueous**.

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