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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 |
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Answer» Solution :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 |
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