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Types of Redox Reactions

A 1g sample...

Question

A $1$ g sample of $H_{2} O_{2}$ solution containing $x %$ $H_{2} O_{2}$ by mass requires x $c m^{3}$ of a $K M n O_{4}$ solution for complete oxidation under acidic condition. Calculate the normality of $K M n O_{4}$ solution.

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Solution

Given, $1 g$ of sample of $H_{2} O_{2}$ has $x$ % $H_{2} O_{2}$ by mass
This means $100 g$ sample has $x$ gm of $H_{2} O_{2}$
$\Rightarrow 1 g$ sample has $\frac{1 g \times x g m}{100 g m} H_{2} O_{2} ⟶ (1)$
Now, Volume of $K M n O_{4}$ used for neutralization= $x c m^{3}$
We know,
At equivalence,
No. of gm equivalents of $H_{2} O_{2}$ =No. of gm equivalents of $K M n O_{4} ⟶ (2)$
$\Rightarrow N_{1} V_{1} H_{2} O_{2} = N_{2} V_{2} K M n O_{4}$
$\Rightarrow \frac{x}{100 \times 17} = \frac{N_{i} X}{1000}$ $[∵ N o r m a l i t y = \frac{W t}{E q . W t} 1000 V i n m l]$
$[E q u i v a l e n t W e i g h t o f H_{2} O_{2} = \frac{34}{2} = 17]$
$\Rightarrow N_{2} = \frac{10}{17} = 0.588 N$
$∴$ Normality of $K M n O_{4} = 0.588 N$

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