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

Answer

10

Explanation

The balanced ionic equation for the reaction is
`MnO_(4)^(-)+5Fe^(2+)+8H^(+)rarrMn^(2+)+5Fe^(3+)+4H_(2)O`
From the balanced equation, it is evident that 1 mole of `KMnO_(4)-=5` moles of `FeSO_(4)`
Applying molarity equation to the balanced redox equation, we have,
`(M_(1)V_(1))/(n_(1))(KMnO_(4))=(M_(2)V_(2))/(n_(2))(FeSO_(4))`
or `(1xxV_(1))/(8xx1)=(1)/(4)xx(25)/(5)`
or `V_(1)=(1xx25xx8)/(4xx5)=10.0cm^(3)`
Thus,
the volume of `M//8KMnO_(4)` solution required = 10.0mL.