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Hydrogen Peroxide

A solution of...

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A solution of $0.4 g$ sample of $H_{2} O_{2}$ reacted with $0.632 g$ $K M n O_{4}$ in the presence of sulphuric acid. Calculate the percentage purity of sample of $H_{2} O_{2}$ .

79%

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91%

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85%

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68%

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Solution

The correct option is C 85%
$2 K M n O_{4} + 3 H_{2} S O_{4} + 5 H_{2} O_{2} \to K_{2} S O_{4} + 2 M n S O_{4} + 8 H_{2} O + 5 O_{2}$
Eq. wt of $K M n O_{4} = \frac{m o l . w t}{C h a n g e i n O N p e r m o l e} = \frac{158}{5} = 31.6$
Again from the above reaction we see that 2 moles of $K M n O_{4}$ combines with 5 moles of $H_{2} O_{2}$
or 10 equivalents (2 moles) of $K M n O_{4}$ combines with 5 moles of $H_{2} O_{2}$
or 1 equivalent of $K m n O_{4}$ combines with 0.5 moles of $H_{2} O_{2}$
Equivalent weight of $H_{2} O_{2} = \frac{m o l . w t .}{2} = \frac{34}{2}$
eq of $H_{2} O_{2} =$ eq of $K M n O_{4}$
Let $x$ be the mass of $H_{2} O_{2}$ in $g$
$\frac{x}{17} = \frac{0.632}{31.6}$
$x = 0.34 g$
% Purity = $\frac{0.34}{0.4} \times 100 = 85 %$

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Similar questions

Q. A solution of a

0.4

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H_{2} O_{2}

reacted with

0.632

g of

K M n O_{4}

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Hydrogen Peroxide

Standard XII Chemistry

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A solution of 0.4 g sample of H2O2 reacted with 0.632 g KMnO4 in the presence of sulphuric acid. Calculate the percentage purity of sample of H2O2.

A solution of $0.4 g$ sample of $H_{2} O_{2}$ reacted with $0.632 g$ $K M n O_{4}$ in the presence of sulphuric acid. Calculate the percentage purity of sample of $H_{2} O_{2}$ .