A solution of ferrous oxalate has been prepared by dissolving 3.6 g `L^(-1)` calculate the volume of 0.01 M `KMnO_(4)` solution required for complete oxidation of 100 mL of ferrous oxalate solution in acidic medium

Answer

150 mL

Explanation

Molarity of `FeC_(2)O_(4)` solution `=("mass in" gL^(-1))/("Mol mass in" g mol^(-1))=(3.6)/(144)=0.025M`
The balanced chemical equation for the redox reaction is :
`5FeC_(2)O_(4)+3MinO_(4)^(2-)+24H^(+)rarr5Fe^(3+)+3Mn^(2+)10CO_(2)+12H_(2)O`
Applying molarity equation we have
`(0.01xxV)/(3)(MnO_(4)^(-))=(0.025xx100)/(5)(FeC_(2)O_(4)) "in" V=(0.025xx100xx3)/(5xx0.01)=150 mL`