Determine the volume of `M//8 KMnO_(4)` solution required to react completely with 25.0 `cm^(3)` of `M//4 FeSO_(4)` solution in acidic medium

Explanation

The balanced ionic equation for the reaction is `MnO_(4)^(-)+5Fe^(2+)+8 H^(+) rarr Mn^(2+)+5Fe^(3+)+4 H_(2)O`
From the balced equation it is evident that 1 mole of `KmnO_(4)=5` moles of `FeSO_(4)`
Applying molarity eqaution to the balced redox equation we have
`(M_(1)V_(1))/(n_(1))(KMnO_(4))=(M_(2)V_(2))/(n_(2))(FeSO_(4)) or (1xxV)/(8xx1)=1/4xxx25/5 or V_(1)=(1xx25xx8)/(4xx5)=10.0 cm^(3)`
thus th volume of `M/8 KnnO_(74)` solution required =10.0 mL