A sample ( 5.6 g ) containing iron is completely dissolved in cold dilute HCl to prepare a 250 mL of

Question

A sample ( 5.6 g ) containing iron is completely dissolved in cold dilute HCl to prepare a 250 mL of solution. Titration of 25.0 mL of this solution requires 12.5 mL of $0.03 \mathrm{M} \mathrm{KMnO}_4$ solution to reach the end point. Number of moles of $\mathrm{Fe}^{2+}$ present in 250 mL solution is $x 	imes 10^{-2}$ (consider complete dissolution of $\mathrm{FeCl}_2$ ). The amount of iron present in the sample is $y \%$ by weight.
(Assume : $\mathrm{KMnO}_4$ reacts only with $\mathrm{Fe}^{2+}$ in the solution Use : Molar mass of iron as $56 \mathrm{~g} \mathrm{~mol}^{-1}$ )

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