During estimation of oxalic acid Vs `KMnO_(4)`, self indicator is

Options

A. `KMnO_(4)`
B. oxalic acid
C. `K_(2)SO_(4)`
D. `MnSO_(4)`

Answer

To solve the question regarding the self-indicator used during the estimation of oxalic acid with potassium permanganate (KMnO4), we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Reaction**:
- When estimating oxalic acid (C2H2O4) using KMnO4, we recognize that KMnO4 is a strong oxidizing agent. The reaction takes place in an acidic medium, usually with sulfuric acid (H2SO4).

2. **Identifying the Components**:
- The components involved in the titration are:
- Oxalic acid (C2H2O4)
- Potassium permanganate (KMnO4)
- Sulfuric acid (H2SO4)

3. **Writing the Reaction**:
- The balanced chemical reaction for the titration can be written as follows:
\[ 2 KMnO_4 + 5 C_2H_2O_4 + 6 H_2SO_4 \rightarrow K_2SO_4 + 2 MnSO_4 + 8 H_2O + 10 CO_2 \]
- In this reaction, KMnO4 is reduced, and oxalic acid is oxidized.

4. **Identifying the Self-Indicator**:
- In this titration, KMnO4 itself acts as a self-indicator. The last drop of KMnO4 added to the solution will impart a pink color, indicating the endpoint of the titration.

5. **Conclusion**:
- Therefore, the self-indicator during the estimation of oxalic acid using KMnO4 is potassium permanganate (KMnO4).

### Final Answer:
The self-indicator during the estimation of oxalic acid versus KMnO4 is **KMnO4**.

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