When `Cl_(2)` water is added to a salt solution containing chloroform, chloroform layer turns violet. Salt contains

Options

A. `Cl^(-)`
B. `I^(-)`
C. `NO_(3)^(-)`
D. `S^(2-)`

Explanation

To solve the question, we need to determine which salt is present in the solution that causes the chloroform layer to turn violet when chlorine water is added. The key is to understand the reactions that take place when chlorine interacts with halide ions.

### Step-by-Step Solution:

1. **Identify the Components**:
- We have chlorine water (Cl₂ in water) and a salt solution containing chloroform (CHCl₃).
- The salt is likely to contain halide ions (e.g., Cl⁻, Br⁻, I⁻).

2. **Understand Chlorine's Reactivity**:
- Chlorine (Cl₂) is a strong oxidizing agent and is highly electronegative. It can displace other halides from their salts.
- The halides of interest here are bromide (Br⁻) and iodide (I⁻).

3. **Reactions with Halides**:
- When Cl₂ is added to a solution containing bromide ions (Br⁻), it can oxidize Br⁻ to bromine (Br₂), which is brown in color.
- When Cl₂ is added to a solution containing iodide ions (I⁻), it can oxidize I⁻ to iodine (I₂), which is violet in color.

4. **Analyze the Color Change**:
- The problem states that the chloroform layer turns violet upon the addition of chlorine water. This indicates that iodine (I₂) is produced in the reaction.
- Therefore, the salt must contain iodide ions (I⁻).

5. **Conclusion**:
- Based on the above analysis, the salt in the solution must contain iodide ions (I⁻) because the formation of iodine leads to the violet color observed in the chloroform layer.

### Final Answer:
The salt contains iodide ions (I⁻).

---