How many millilitres of a $0.05 \mathrm{~M} \mathrm{~KMnO}_4$ solution are required to oxide $2.0 \mathrm{~g}$ of $\mathrm{FeSO}_4$ in a dilute acid solution? $(\mathrm{Fe}=56, \mathrm{S}=32, \mathrm{O}=16)$.

JEE CHEMISTRY MCQ: SOME BASIC CONCEPTS OF CHEMISTRY

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Application +4 | -1

How many millilitres of a

0.05 \mathrm{~M} \mathrm{~KMnO}_4

solution are required to oxide

2.0 \mathrm{~g}

\mathrm{FeSO}_4

in a dilute acid solution?

(\mathrm{Fe}=56, \mathrm{S}=32, \mathrm{O}=16)

View answer and explanation

Correct option: A

Option A (53) is correct because the volume of KMnO4 required is calculated using stoichiometry and molarity, resulting in approximately 53 mL.

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