A: Copper rod turns colourless solution of zinc sulphate to blue.
R: Zinc reduce `Cu^(2+) " ions to " Cu^(+)`

Options

A. If both Assertion & Reason are true and the reason is the correct explanation of the assertion, then mark (1)
B. If both Assertion & Reason are true but the reason is not the correct explanation of the assertion, then mark (2)
C. If Assertion is true statement but Reason is false, then mark (3)
D. If both Assertion and Reason are false statements then mark (4)

Answer

To solve the question, we need to analyze both the assertion (A) and the reason (R) provided in the statement.

**Step 1: Analyze the Assertion (A)**
The assertion states that "Copper rod turns colorless solution of zinc sulfate to blue."
- Zinc sulfate (ZnSO4) is a colorless solution.
- Copper sulfate (CuSO4) is a blue solution.
- When a copper rod is placed in a colorless zinc sulfate solution, there is no reaction that would turn the solution blue. Instead, the copper rod would not change the color of the solution, as zinc is more reactive than copper.

**Conclusion:** The assertion is **false**.

**Step 2: Analyze the Reason (R)**
The reason states that "Zinc reduces Cu²⁺ ions to Cu⁺."
- In the electrochemical series, zinc (Zn) is more reactive than copper (Cu).
- When zinc is in contact with copper ions (Cu²⁺), zinc will displace copper from the solution, reducing Cu²⁺ to Cu (not Cu⁺). The reaction can be represented as:
\[ \text{Zn} + \text{Cu}^{2+} \rightarrow \text{Zn}^{2+} + \text{Cu} \]
- The reduction of Cu²⁺ to Cu does not involve the formation of Cu⁺.

**Conclusion:** The reason is also **false**.

**Final Conclusion:** Both the assertion and the reason are false.

**Answer:** The correct option is that both A and R are false.

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