Question

Calculate the total volume of $0.1$ molar $KMn{O}_4$ solution that is needed to oxidized 100 mg of each furious oxalate and furious sulphate in a mixture in acidic medium.

• A. 1.096 ml
• B. 1.32 ml
• C. 5.48 ml
• D. None of these

Answer 1

The correct option is C 5.48 ml

m-eq. of $KMn{O}_4$ = m-eq. of $Fe{C}_2{O}_4$ + m-eq. of $FeS{O}_4$
$(0.1\times 5)\times V=\frac{100}{\frac{144}{3}}+\frac{100}{\frac{152}{1}}$
$V=5.48mL$