The number of moles of $H_{2} O_{2}$ required to completely react with $400 m l$ of $.5 N K M n O_{4}$ is acidic medium are:

0.1

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0.2

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1.0

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0.5

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Solution

The correct option is A $0.1$
$n_{f a c t o r}$ of $H_{2} O_{2} = 2$
$n_{f a c t o r}$ of $K M n O_{4} = 5$
Equivalent of $H_{2} O_{2} =$ Equivalent of $K M n O_{4}$
Let the number of moles of $H_{2} O_{2}$ be $x$
$⟹ x \times 2 = 400 \times 0.5$
$⟹ x \times 2 = 200$
$⟹ x = 100$ $m i l l i m o l e s = 0.1$ $m o l e s$

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The number of moles of H2O2 required to completely react with 400 ml of .5N KMnO4 is acidic medium are:

The correct option is A 0.1nfactor of H2O2=2nfactor of KMnO4=5Equivalent of H2O2= Equivalent of KMnO4Let the number of moles of H2O2 be x⟹x×2=400×0.5⟹x×2=200⟹x=100 millimoles=0.1 moles

The number of moles of $H_{2} O_{2}$ required to completely react with $400 m l$ of $.5 N K M n O_{4}$ is acidic medium are: