A piece of iron wire weighing 1.63 g is converted to Fe²⁺(aq) and requires 21.9 mL of KMnO₄ solution for its titration. What is the molarity of the KMnO₄ solution? The reaction occurring during the titration is: 5 Fe²⁺ (aq) + MnO₄^- (aq) + 8 H⁺ (aq) → 5 Fe³⁺(aq) + Mn²⁺ (aq) + 4 H₂O A) 1.33 M B) 0.267 M C) 2.67 × 10^-4 M D) 14.9 M E) 1.33 × 10^-3 M

Question

Quizplus · Accepted Answer

To find the molarity of KMnO₄, first calculate moles of Fe²⁺ using the mass of iron (1.63 g) and its molar mass (55.85 g/mol). Then, use the stoichiometry of the reaction (5 Fe²⁺ per 1 MnO₄⁻) to find moles of KMnO₄. Finally, divide the moles of KMnO₄ by the volume in liters (0.0219 L) to find the molarity.

A Piece of Iron Wire Weighing 1