Assertion: During electrolysis of `CuSO_4`(aq) using copper electrodes, copper is dissolved at anode and deposited at cathode.
Reason: Oxidation takes place at anode and reduction at cathode.

Options

A. Assertion and Reason both are correct statements and reason is the correct explanation of the assertion.
B. Assertion and Reason both are correct statements, but reason is not the correct explanation of the assertion.
C. Assertion is true, but reason is false.
D. Assertion is false, but reason is true.

Explanation

To solve the question regarding the assertion and reason related to the electrolysis of copper sulfate (CuSO₄) using copper electrodes, we can break it down into a step-by-step explanation.

### Step-by-Step Solution:

1. **Understanding Electrolysis**:
- Electrolysis is a process that uses electrical energy to drive a non-spontaneous chemical reaction. In this case, we are using an aqueous solution of copper sulfate (CuSO₄).

2. **Identifying the Electrodes**:
- In the setup, we have two electrodes: an anode (positive electrode) and a cathode (negative electrode). Both electrodes are made of copper.

3. **Dissociation of CuSO₄**:
- When CuSO₄ is dissolved in water, it dissociates into copper ions (Cu²⁺) and sulfate ions (SO₄²⁻). The dissociation can be represented as:
\[ \text{CuSO}_4 \rightarrow \text{Cu}^{2+} + \text{SO}_4^{2-} \]

4. **Movement of Ions**:
- In an electrolytic cell, the positively charged ions (Cu²⁺) will move towards the cathode, while the negatively charged ions (SO₄²⁻) will move towards the anode.

5. **Reactions at the Anode**:
- At the anode, oxidation occurs. Since the anode is made of copper, the copper from the anode will dissolve into the solution. The oxidation reaction can be represented as:
\[ \text{Cu (s)} \rightarrow \text{Cu}^{2+} + 2\text{e}^- \]
- This confirms the assertion that copper is dissolved at the anode.

6. **Reactions at the Cathode**:
- At the cathode, reduction occurs. The Cu²⁺ ions from the solution gain electrons and are deposited as solid copper. The reduction reaction can be represented as:
\[ \text{Cu}^{2+} + 2\text{e}^- \rightarrow \text{Cu (s)} \]
- This confirms the assertion that copper is deposited at the cathode.

7. **Conclusion**:
- Both the assertion and reason are correct. The assertion states that during the electrolysis of CuSO₄ using copper electrodes, copper is dissolved at the anode and deposited at the cathode. The reason explains that oxidation occurs at the anode and reduction at the cathode, which is the correct explanation for the assertion.

### Final Answer:
- Both the assertion and reason are correct, and the reason is a correct explanation of the assertion.