Question Stem
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 M $$KMnO_4$$ solution to reach the end point. Number of moles of Fe$$^{2+}$$ present in 250 mL solution is $$x \times 10^{−2}$$ (consider complete dissolution of $$FeCl_2$$). The amount of iron present in the sample is y% by weight.
(Assume: $$KMnO_4$$ reacts only with Fe$$^{2+}$$ in the solution
Use: Molar mass of iron as 56 g mol$$^{−1}$$)