When an aqueous solution of `LiCl` is electrolyzed using graphite electrodes, as the current flows, the `pH` of the solution around cathode `……………………`

Explanation

To solve the question regarding the change in pH of an aqueous solution of LiCl during electrolysis, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Ions in the Solution**:
- When LiCl is dissolved in water, it dissociates into four types of ions: Li⁺, Cl⁻, H⁺, and OH⁻.
- The relevant ions for electrolysis are Li⁺ and H⁺ (cations) and Cl⁻ and OH⁻ (anions).

2. **Determine the Electrolysis Process**:
- During electrolysis, cations migrate towards the cathode (negative electrode) where reduction occurs.
- The two cations present are Li⁺ and H⁺.

3. **Compare the Reduction Potentials**:
- The standard reduction potential for H⁺ to H₂ is higher than that for Li⁺ to Li.
- Therefore, H⁺ will be reduced at the cathode instead of Li⁺.

4. **Reduction Reaction**:
- The reduction of H⁺ at the cathode can be represented by the following half-reaction:
\[ 2H^+ + 2e^- \rightarrow H_2(g) \]
- This reaction produces hydrogen gas and consumes H⁺ ions from the solution.

5. **Effect on H⁺ Concentration**:
- As H⁺ ions are reduced to form hydrogen gas, the concentration of H⁺ ions in the solution decreases.

6. **Impact on pH**:
- pH is defined as:
\[ \text{pH} = -\log[H^+] \]
- Since the concentration of H⁺ ions is decreasing, the pH of the solution will increase.

### Conclusion:
- Therefore, as the current flows during the electrolysis of an aqueous solution of LiCl, the pH of the solution around the cathode **increases**.

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