Question

Calculate the volume of 0.05m kmno4 solution required to oxide 2g of feso4

Answer 1

KMnO4 is reduced to Mn2+ so FeSO4 is oxidised to Fe3+. hence the equation required is KMnO4 +5 FeSO4= Mn2+ +5Fe3+ + ions so number of moles in 2g of FeSO4 is 2/(56+32+64)=2/152 moles 2/152 =0.05 × v hence v=2/7.6 L =263 mL approximately