Which of the following compounds (s) undergo disproportionation in aqueous solution ?

Options

A. `TlCl_(3)`
B. `GaCl`
C. `InCL`
D. `TlCl`

Explanation

To determine which of the given compounds undergo disproportionation in aqueous solution, we need to analyze the oxidation states of the elements in each compound and their stability. Disproportionation is a reaction in which a single substance is simultaneously oxidized and reduced, forming two different products.

### Step-by-Step Solution:

1. **Identify the Compounds**:
Let's assume the compounds in question are:
- A) TiCl3
- B) GaCl
- C) InCl
- D) TlCl

2. **Analyze the Oxidation States**:
- For **TiCl3**: Titanium (Ti) is in the +3 oxidation state. The +1 oxidation state (TiCl) is more stable for thallium due to the inert pair effect. Thus, TiCl3 does not undergo disproportionation.
- For **GaCl**: Gallium (Ga) in GaCl is in the +1 oxidation state. It can disproportionate to form elemental Ga and GaCl3, where Ga is in the +3 oxidation state.
- For **InCl**: Indium (In) in InCl is also in the +1 oxidation state. Similar to GaCl, it can disproportionate to form elemental In and InCl3, where In is in the +3 oxidation state.
- For **TlCl**: Thallium (Tl) in TlCl is in the +1 oxidation state. The +3 oxidation state is less stable, and TlCl does not undergo disproportionation.

3. **Conclusion**:
- Based on the analysis, **GaCl** and **InCl** undergo disproportionation in aqueous solution, while **TiCl3** and **TlCl** do not.

### Final Answer:
The compounds that undergo disproportionation in aqueous solution are **B) GaCl** and **C) InCl**.