\(x\) mL of \(0.05\,M\) \(KMnO_4\) solution is required to oxidise completely \(1.52\) g of \(FeSO_4\) in acidic medium. The value of \(x\) is
\[
(\text{Atomic weights: } Fe=56,\ S=32,\ O=16)
\]
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For \(KMnO_4\) in acidic medium:
\[
n\text{-factor}=5
\]
\[
N=M\times5.
\]
For redox titrations:
\[
\boxed{N_1V_1=N_2V_2}
\]
or equivalently,
\[
\boxed{\text{Equivalents of oxidant}=\text{Equivalents of reductant}}
\]