Copper can be reduced from acidic copper sulphate solution by

Options

A. Silver
B. Iron
C. Carbon
D. Lead

Answer

To solve the question of how copper can be reduced from an acidic copper sulfate solution, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Reaction Context**:
- We start with an acidic copper sulfate solution, which contains copper ions (Cu²⁺) in a +2 oxidation state.

2. **Reduction Process**:
- Reduction involves the gain of electrons. In this case, Cu²⁺ ions will gain two electrons to become metallic copper (Cu) in a 0 oxidation state:
\[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \]

3. **Identifying the Reducing Agent**:
- To reduce Cu²⁺ to Cu, we need a reducing agent (a metal that can donate electrons). The reducing agent must have a higher tendency to oxidize (lose electrons) than copper.

4. **Analyzing the Given Metals**:
- We have four options: silver (Ag), iron (Fe), carbon (C), and lead (Pb). We need to compare their reduction potentials with that of copper.
- The standard reduction potential (E°) values indicate how easily a species can be reduced. A lower reduction potential means a greater tendency to oxidize.

5. **Reduction Potentials**:
- The reduction potential of copper (Cu²⁺/Cu) is +0.34 V.
- We need to check the reduction potentials of the other metals:
- Silver (Ag) has a higher reduction potential than copper.
- Carbon (C) has a higher reduction potential than copper.
- Lead (Pb) has a higher reduction potential than copper.
- Iron (Fe) has a lower reduction potential than copper.

6. **Conclusion**:
- Since iron (Fe) has a lower reduction potential than copper, it can effectively donate electrons to reduce Cu²⁺ to Cu. Therefore, iron is the suitable reducing agent in this reaction.
- The overall reaction can be summarized as:
\[ \text{Cu}^{2+} + \text{Fe} \rightarrow \text{Fe}^{2+} + \text{Cu} \]

### Final Answer:
Copper can be reduced from acidic copper sulfate solution by **iron (Fe)**.

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