The increase in the molar conductivity of `HCl` with dilution is due to

Options

A. Increase in the self ionization of water
B. Hydrolysis of `HCl`
C. Decrease in the self ionization of water
D. Decrease in the interionic forces.

Explanation

To solve the question regarding the increase in the molar conductivity of HCl with dilution, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Molar Conductivity**:
Molar conductivity (\( \Lambda_m \)) is defined as the conductivity of an electrolyte solution divided by its molar concentration. It indicates how well an electrolyte can conduct electricity in solution.

2. **Effect of Dilution**:
When an electrolyte like HCl is diluted, its concentration decreases. According to the Debye-Hückel-Onsager equation, the molar conductivity of a strong electrolyte increases with dilution.

3. **Ionization of HCl**:
HCl dissociates completely in water into H\(^+\) and Cl\(^-\) ions. When diluted, the number of water molecules increases, which can lead to a reduction in the interionic forces between the ions.

4. **Interionic Forces**:
In concentrated solutions, the ions are closer together, and the attractive forces between them can hinder their movement. As the solution is diluted, these interionic forces decrease, allowing the ions to move more freely.

5. **Increased Mobility of Ions**:
With the decrease in interionic forces, the mobility of H\(^+\) and Cl\(^-\) ions increases. Higher mobility means that the ions can move more easily through the solution, which contributes to an increase in molar conductivity.

6. **Conclusion**:
Therefore, the increase in the molar conductivity of HCl with dilution is primarily due to the decrease in interionic forces, which enhances the mobility of the ions.

### Final Answer:
The increase in the molar conductivity of HCl with dilution is due to the **decrease in interionic forces**.

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