What is the normality of a $K M n O_{4}$ solution in which $15.8 g$ of $K M n O_{4}$ is present in $250 m L$ solution and the solution is used as an oxidant, where ${M n O_{4}}^{-}$ is reduced to ${M n}^{2 +}$ ? (Given: molar mass of $K M n O_{4} = 158 g m o l^{- 1}$ )

K M n O_{4}

(mol. Wt

= 158

) oxidizes acid in acidic medium to

C O_{2}

and water as follows.

5 C_{2} O_{4}^{2 -} + 2 M n O^{-} + 16 H^{+} \to 10 C O_{2} + 2 M n^{2 +} + 8 H_{2} O

What is the equivalent weight of

K M n O_{4}

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How many gram of KMnO4 is contained in 4 litre of 0.05N solution. The KMnO4 is to used as an oxidant in acid medium (MW=158):

The correct option is C 6.32gEquivalentmass=Molarmassn−factorIn acidic medium, M+7n gets converted to M+2n state ∴n−factor=5∴Equivalentmass=1585=31.6Now, Normality=Mass/EquivalentmassVolumeofsolution(inlitres)∴0.05=Mass31.6×4∴ Mass=6.32g

How many gram of ${K M n O}_{4}$ is contained in $4$ litre of $0.05 N$ solution. The ${K M n O}_{4}$ is to used as an oxidant in acid medium $(M_{W} = 158) :$