What volume of `0.1` M `KMnO_4` is required to oxidise 100 " mL of " 0.2 M `FeSO_4` in acidic medium ? The reaction involved is

Explanation

To solve the problem of determining the volume of `0.1 M KMnO4` required to oxidize `100 mL` of `0.2 M FeSO4` in acidic medium, we will follow these steps:

### Step 1: Write the balanced chemical equation
The balanced chemical equation for the reaction between `FeSO4` and `KMnO4` in acidic medium is:
\[ 10 \text{FeSO}_4 + 2 \text{KMnO}_4 + 8 \text{H}_2\text{SO}_4 \rightarrow 5 \text{Fe}_2(\text{SO}_4)_3 + 2 \text{MnSO}_4 + \text{K}_2\text{SO}_4 + 8 \text{H}_2\text{O} \]
From this equation, we can see that 10 moles of `FeSO4` react with 2 moles of `KMnO4`.
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