`FeC_(2)O_(4)` can decolorise acidified `KMnO_(4)` due to the oxidation of (a) _____and (b)____.

Answer

To solve the question regarding the decolorization of acidified KMnO4 by FeC2O4 (ferrous oxalate), we need to identify the species that are oxidized in the reaction.

### Step-by-Step Solution:

1. **Understanding the Reaction**:
- Acidified KMnO4 is a strong oxidizing agent. In acidic conditions, it can oxidize various substances, including ferrous ions (Fe²⁺) and oxalate ions (C₂O₄²⁻).

2. **Identifying the Oxidized Species**:
- The first species that gets oxidized is the **ferrous ion (Fe²⁺)**. It is oxidized to **ferric ion (Fe³⁺)**.
- The second species that gets oxidized is the **oxalate ion (C₂O₄²⁻)**. It is oxidized to **carbon dioxide (CO₂)**.

3. **Writing the Half-Reactions**:
- For the oxidation of ferrous ions:
\[ \text{Fe}^{2+} \rightarrow \text{Fe}^{3+} + e^- \]
- For the oxidation of oxalate ions:
\[ \text{C}_2\text{O}_4^{2-} \rightarrow 2\text{CO}_2 + 2e^- \]

4. **Combining the Half-Reactions**:
- When these half-reactions are combined with the reduction half-reaction of KMnO4, we can see that the overall reaction leads to the decolorization of KMnO4 due to the reduction of MnO4⁻ to Mn²⁺.

5. **Conclusion**:
- Therefore, the two species that are oxidized in the reaction are:
- (a) **Ferrous ions (Fe²⁺)**
- (b) **Oxalate ions (C₂O₄²⁻)**

### Final Answer:
FeC₂O₄ can decolorize acidified KMnO₄ due to the oxidation of (a) **Ferrous ions (Fe²⁺)** and (b) **Oxalate ions (C₂O₄²⁻)**.