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Hydrogen Peroxide

If 10 ml of...

Question

If $10$ ml of $H_{2} O_{2}$ solution requires $25$ ml of $\frac{N}{20} K M n O_{4}$ for complete oxidation in acidic medium, then the mass (in g) of available $O_{2}$ per litre present in the solution is:

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Solution

The correct option is A $2$
The oxidation reaction is as follows:
$2 K M n O_{4} + 5 H_{2} O_{2} + 4 H_{2} {S O}_{4} \to 2 {K H S O}_{4} + 2 M n S O_{4} + 8 H_{2} O + 5 O_{2}$
Meq. of $O_{2} =$ Meq. of $H_{2} O_{2} =$ Meq. of $K M n O_{4}$
It is given that $10$ ml of $H_{2} O_{2}$ solution when treated with $25$ ml of $\frac{N}{20} K M n O_{4}$ for complete oxidation.
$N \times 10 = 25 \times \frac{1}{20}$
Normality of $H_{2} O_{2} = 0.125 N =$ Normality of $O_{2}$
Weight of $O_{2} = 0.125 \times 32 = 4$ g per litre.

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If 10 ml of H2O2 solution requires 25 ml of N20KMnO4 for complete oxidation in acidic medium, then the mass (in g) of available O2 per litre present in the solution is:

If $10$ ml of $H_{2} O_{2}$ solution requires $25$ ml of $\frac{N}{20} K M n O_{4}$ for complete oxidation in acidic medium, then the mass (in g) of available $O_{2}$ per litre present in the solution is: