Which of the following displaces `Br_(2)` from an aqueous solution containing bromide ions ?

Options

A. `I_(2)`
B. `I_(3)^-`
C. `Cl_(2)`
D. `Cl^(-)`

Answer

To determine which of the given options can displace \( \text{Br}_2 \) from an aqueous solution containing bromide ions (\( \text{Br}^- \)), we need to analyze the reactivity of the halogens involved.

### Step-by-Step Solution:

1. **Understand the Reactivity Series of Halogens**:
The halogens are arranged in a reactivity series based on their ability to displace each other. The order of reactivity from highest to lowest is:
- Fluorine (F)
- Chlorine (Cl)
- Bromine (Br)
- Iodine (I)

2. **Identify the Options**:
The options given are:
- \( \text{I}_2 \)
- \( \text{I}_3^- \)
- \( \text{Cl}_2 \)
- \( \text{Cl}^- \)

3. **Analyze Each Option**:
- **\( \text{I}_2 \)**: Iodine is less reactive than bromine, so it cannot displace \( \text{Br}_2 \).
- **\( \text{I}_3^- \)**: This is a polyatomic ion that contains iodine. Since iodine is less reactive than bromine, it will also not displace \( \text{Br}_2 \).
- **\( \text{Cl}_2 \)**: Chlorine is more reactive than bromine and can displace \( \text{Br}_2 \) from the solution. The reaction can be represented as:
\[ \text{Cl}_2 + 2 \text{Br}^- \rightarrow 2 \text{Cl}^- + \text{Br}_2 \]
- **\( \text{Cl}^- \)**: Chloride ion is less reactive than bromine and cannot displace \( \text{Br}_2 \).

4. **Conclusion**:
Based on the reactivity series, the only species that can displace \( \text{Br}_2 \) from an aqueous solution containing bromide ions is \( \text{Cl}_2 \).

Thus, the correct answer is **option 3: \( \text{Cl}_2 \)**.