Hydroxylamine reduce iron (III) according to the equation :
`2NH_(2)OH + 4 Fe^(3+) rarr N_(2)O(g)uarr + H_(2)O + 4Fe^(2+) + 4H^(+)`
Iron (II) thus produced is estimated by titration with a standard permanganate solution. The reaction is
`MnO_(4)^(-) + 5 Fe^(2+) + 8H^(+) rarr Mn^(2+) + 5Fe^(3+) + 4H_(2)O`
A 10 mL sample of hydroxylamine solution was diluted to 1 litre. 50 mL of this diluted solution was boiled with an excess of iron (III) solution. The resulting solution required 12 mL of 0.02 M `KMnO_(4)` solution for complete oxidation of iron (II). Calculate the weight of hydroxylamine in one litre of the original solution

Explanation

To solve the problem step-by-step, we will follow the procedure outlined in the video transcript and derive the weight of hydroxylamine in one liter of the original solution.

### Step 1: Calculate the moles of KMnO4 used
Given that 12 mL of 0.02 M KMnO4 solution is used, we can calculate the moles of KMnO4.

\[ \text{Moles of KMnO}_4 = \text{Molarity} \times \text{Volume (in L)} \]
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