The solublity of `KCl` is relatively more in :

Options

A. `C_6 H_6 (D =0)`
B. `(CH-3)_2 CO(D=2)`
C. ` CH_3OH(D=32)`
D. `C Cl_4(D=0)`

Explanation

To determine the solvent in which potassium chloride (KCl) is more soluble, we need to consider the polarity of both the solute (KCl) and the solvents provided. KCl is an ionic compound, consisting of K⁺ and Cl⁻ ions, which makes it a polar solute. Polar solutes tend to dissolve better in polar solvents due to the principle of "like dissolves like."

### Step-by-Step Solution:

1. **Identify the Solute**:
- The solute in this case is potassium chloride (KCl), which is an ionic compound and therefore polar.

2. **List the Solvents**:
- The solvents provided are:
- Benzene (C₆H₆)
- Acetone (CH₃COCH₃)
- Ethanol (C₂H₅OH)
- Carbon tetrachloride (CCl₄)

3. **Determine the Polarity of Each Solvent**:
- **Benzene (C₆H₆)**: Non-polar (dipole moment = 0)
- **Acetone (CH₃COCH₃)**: Polar (dipole moment ≈ 2.88 D)
- **Ethanol (C₂H₅OH)**: Polar (dipole moment ≈ 1.69 D)
- **Carbon tetrachloride (CCl₄)**: Non-polar (dipole moment = 0)

4. **Compare the Polarity of the Solvents**:
- Among the solvents, benzene and carbon tetrachloride are non-polar, while acetone and ethanol are polar.
- Between acetone and ethanol, acetone has a higher dipole moment, indicating it is more polar than ethanol.

5. **Conclusion**:
- Since KCl is a polar solute, it will be more soluble in a polar solvent. Among the solvents listed, acetone has the highest polarity.
- Therefore, the solubility of KCl is relatively more in **acetone**.

### Final Answer:
The solubility of KCl is relatively more in **acetone (CH₃COCH₃)**.