Calculate the volume of 10 volume `H_2 O_2` required to neutralise 200 mL of 2N `KMnO_4` in acidic medium.

Explanation

To calculate the volume of 10 volume hydrogen peroxide (H₂O₂) required to neutralize 200 mL of 2N KMnO₄ in acidic medium, we can follow these steps:

### Step 1: Understand the Reaction
In acidic medium, potassium permanganate (KMnO₄) acts as an oxidizing agent and is reduced to manganese(II) ions (Mn²⁺). Hydrogen peroxide (H₂O₂) acts as a reducing agent. The balanced reaction can be represented as:
\[ \text{MnO}_4^- + 5 \text{H}_2\text{O}_2 + 8 \text{H}^+ \rightarrow \text{Mn}^{2+} + 5 \text{O}_2 + 8 \text{H}_2\text{O} \]

From this equation, we see that 1 mole of KMnO₄ reacts with 5 moles of H₂O₂.

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