In the electrolysis of an aqueous potassium sulphate solution, the
`pH` of the solution in the space near an electrode increased.
Which pole of the current source is the electrode connected
to ?

Options

A. The positive pole
B. Could be either polde
C. The negative pole
D. Cannot be determined

Explanation

To determine which pole of the current source the electrode is connected to, we need to analyze the electrolysis of an aqueous potassium sulfate (K2SO4) solution and understand the changes in pH near the electrodes.

### Step-by-Step Solution:

1. **Identify the Electrolysis Process**:
- In the electrolysis of K2SO4, the solution dissociates into K⁺ and SO₄²⁻ ions, along with water (H₂O) which dissociates into H⁺ and OH⁻ ions.

2. **Electrode Reactions**:
- At the **anode** (positive electrode), the reaction involves the discharge of OH⁻ ions:
\[ 4OH^- \rightarrow 2H_2O + O_2 + 4e^- \]
- At the **cathode** (negative electrode), the reaction involves the discharge of H⁺ ions:
\[ 2H^+ + 2e^- \rightarrow H_2 \]

3. **Effect on pH**:
- At the anode, as OH⁻ ions are consumed, their concentration decreases. This leads to a decrease in pOH, which means an increase in pH (since pH + pOH = 14).
- At the cathode, as H⁺ ions are consumed, their concentration decreases, which leads to an increase in pH.

4. **Conclusion**:
- Since the problem states that the pH of the solution near an electrode increased, this indicates that the electrode must be the cathode. Therefore, the electrode is connected to the **negative pole** of the current source.

### Final Answer:
The electrode is connected to the **negative pole** of the current source.

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