A sample (5.6 g) containing iron is completely dissolved in cold dilute HCl to prepare 250 mL of solution. Titration of 25.0 mL of this solution requires 12.5 mL of 0.03 M KMnO₄ solution to reach the end point. Number of moles of Fe²⁺ present in 250 mL solution is x × 10⁻² (consider complete dissolution of FeCl₂). The amount of iron present in the sample is y% by weight. Assume KMnO₄ reacts only with Fe²⁺ in the solution. Use molar mass of iron as 56 g mol⁻¹.
The value of x is ___.