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Hydrogen Peroxide

A 20 mL solut...

Question

A $20 m L$ solution of hydrogen peroxide reacts quantitatively with a $20 m L$ solution of $K M n O_{4}$ acidified with dilute $H_{2} S O_{4} .$ The same volume of the $K M n O_{4}$ solution is decolourized by $10 m L$ of $M n S O_{4}$ in neutral medium simultaneously forming a dark brown precipitate of hydrated $M n O_{2} .$ The brown precipitate is dissolved in $20 m L$ of $0.2 M$ sodium oxalate under boiling condition in the presence of dilute $H_{2} S O_{4} .$ Calculate the volume strength of $H_{2} O_{2} .$

A

4.48

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B

44.8

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C

22.4

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D

2.24

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Solution

The correct option is D $2.24$
$2 K M n O_{4} + 5 H_{2} O_{2} + 3 H_{2} S O_{4} \to 2 M n S O_{4} + K_{2} S O_{4} + 8 H_{2} O + 5 O_{2}$
$2 K M n O_{4} + 3 M n S O_{4} + 2 H_{2} O \to 5 M n O_{2} + 2 H_{2} S O_{4} + K_{2} S O_{4}$
$M n O_{2} + N a_{2} C_{2} O_{4} + 2 H_{2} S O_{4} \to M n S O_{4} + N A_{2} S O_{4} + 2 H_{2} O + 2 C O_{2}$

$∴ Milliequivalents of M n O_{2} = Milliequivalents of N a_{2} C_{2} O_{4} = Milliequivalents of K M n O_{4} = Milliequivalents of H_{2} O_{2} = 20 \times 0.2 \times 2 = 8$

$∴ N_{H_{2} O_{2}} \times 20 = 8$
$N_{H_{2} O_{2}} = 0.4$

$Volume strength of H_{2} O_{2} = 5.6 \times N_{H_{2} O_{2}}$
$= 5.6 \times 0.4 = 2.24$

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