When `CS_(2)` layer containing both `Br_(2)` and `I_(2)` is shaken with excess of `Cl_(2)` water, the violet colour due to `I_(2)` disappears and appereance of pale yellow colour is due to the formation of :

Options

A. `I_(3)^(Θ)` and `Br_(2)` respectively
B. `HIO_(3)` and `BrCl` respectively
C. `KI` and `BrCl` respectively
D. `I^(Θ)` and `Br^(Θ)`, respectively

Answer

To solve the problem, we need to analyze the chemical reactions that occur when a layer of carbon disulfide (CS₂) containing both bromine (Br₂) and iodine (I₂) is shaken with excess chlorine water (Cl₂ in water).

### Step-by-Step Solution:

1. **Identify the Color Changes**:
- The initial color due to iodine (I₂) is violet.
- The color that appears after shaking with chlorine water is pale yellow.

2. **Reactions with Chlorine Water**:
- When chlorine (Cl₂) is added to bromine (Br₂), the following reaction occurs:
\[ \text{Br}_2 + \text{Cl}_2 \rightarrow 2 \text{BrCl} \]
Here, bromine reacts with chlorine to form bromine monochloride (BrCl), which is pale yellow in color.

3. **Reaction of Iodine with Chlorine**:
- Iodine (I₂) also reacts with chlorine (Cl₂) in the presence of water:
\[ 2 \text{I}^- + \text{Cl}_2 \rightarrow 2 \text{Cl}^- + \text{I}_2 \]
However, in excess chlorine, iodine can be oxidized to iodate (IO₃⁻):
\[ 2 \text{I}^- + 8 \text{Cl}_2 + 9 \text{H}_2\text{O} \rightarrow 3 \text{IO}_3^- + 16 \text{Cl}^- + 18 \text{H}^+ \]
This reaction leads to the disappearance of the violet color of iodine.

4. **Conclusion**:
- The disappearance of the violet color is due to the formation of iodate (HIO₃) from iodine.
- The appearance of the pale yellow color is due to the formation of bromine monochloride (BrCl).

5. **Final Answer**:
- The correct answer is that the violet color disappears due to the formation of HIO₃ and the pale yellow color is due to the formation of BrCl.