The colloidal sol of `SnCl_(4)` prefers to adsorb : (in excess of HCl)

Options

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

Explanation

To solve the question regarding the colloidal sol of SnCl4 and its preference for adsorption in the presence of excess HCl, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Components**: We have a colloidal solution of SnCl4 and excess HCl. SnCl4 is a tin(IV) chloride compound, and HCl is hydrochloric acid.

2. **Write the Reaction**: When SnCl4 is mixed with excess HCl, the reaction can be represented as:
\[ \text{SnCl}_4 + \text{HCl} \rightarrow \text{SnCl}_4 + \text{Cl}^- + \text{H}^+ \]
Here, the presence of excess HCl leads to the dissociation of HCl, contributing Cl^- ions and H+ ions into the solution.

3. **Analyze Stability**: The colloidal sol of SnCl4 is unstable in the presence of Cl^- ions. The presence of Cl^- ions in excess can lead to the destabilization of the colloidal particles.

4. **Identify the Adsorbed Species**: In colloidal systems, ions or molecules from the surrounding medium can adsorb onto the surface of the colloidal particles. In this case, the Cl^- ions are likely to adsorb onto the surface of the SnCl4 colloidal particles due to their negative charge.

5. **Conclusion**: Based on the analysis, we can conclude that the colloidal sol of SnCl4 prefers to adsorb Cl^- ions when in excess of HCl.

### Final Answer:
The colloidal sol of SnCl4 prefers to adsorb **Cl^- ions**.

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