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Oxidising Reagent and Reducing Reagent

A 3.4 g sampl...

Question

A $3.4 g$ sample of $H_{2} O_{2}$ solution that has $x % H_{2} O_{2}$ by mass requires $x mL$ of $K M n O_{4}$ solution for complete oxidation under acidic conditions. The molarity of the $K M n O_{4}$ solution is :

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0.5

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0.4

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0.2

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Solution

The correct option is C 0.4
In acidic conditions:
$M n^{7 +} \Rightarrow M n^{2 +}$
$H_{2}^{+ 1} O_{2}^{- 2} \Rightarrow H_{2} O + O_{2}$
$n_{f} o f H_{2} O_{2} = 2$
$n_{f} o f K M n O_{4} = 5$
and we know that:
$(n \times n_{f})_{H_{2} O_{2}} = (n \times n_{f})_{K M n O_{4}}$
$N o r m a l i t y = M o l a r i t y \times n_{f}$
$M o l a r i t y = 0.4$

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A 3.4g sample of H2O2 solution that has x% H2O2 by mass requires x mL of KMnO4 solution for complete oxidation under acidic conditions. The molarity of the KMnO4 solution is :

The correct option is C 0.4In acidic conditions: Mn7+⇒Mn2+ H+12O−22⇒H2O+O2 nf of H2O2=2 nf of KMnO4=5 and we know that: (n×nf)H2O2=(n×nf)KMnO4 Normality=Molarity×nf Molarity=0.4

A $3.4 g$ sample of $H_{2} O_{2}$ solution that has $x % H_{2} O_{2}$ by mass requires $x mL$ of $K M n O_{4}$ solution for complete oxidation under acidic conditions. The molarity of the $K M n O_{4}$ solution is :