Hydroxylamine reduces `Fe^(3+)` accoeding to the following reaction:
`2NH_2OH+4Fe^(3+)toH_2O+4Fe^(2+)+4H^(o+)+N_2O`
`Fe^(2+)` produced is is estimated by titration with `KMnO_4` solution A 10 mL sample of `NH_2OH` is diluted to 1000 mL. 50 " mL of " this diluted sample is boiled with excess of Fe (III) solution. The resulting solution required 12 " mL of " 0.02 M `KMnO_4` for complete oxidation. Determine the strength of `NH_2OH`.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Write the balanced equation for the reaction with KMnO4
The balanced equation for the titration of Fe²⁺ with KMnO₄ is:
\[ \text{MnO}_4^- + 8 \text{H}^+ + 5 \text{Fe}^{2+} \rightarrow \text{Mn}^{2+} + 4 \text{H}_2\text{O} + 5 \text{Fe}^{3+} \]

### Step 2: Calculate the normality of KMnO4 solution
Given that 12 mL of 0.02 M KMnO₄ solution is used:
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