The ion MnO₄^- is often used to analyze for the Fe²⁺ content of an aqueous solution by using the reaction
MnO₄^- + Fe²⁺ → Fe³⁺ + Mn²⁺
In acidic solution. A 45.6-mL sample of a solution containing Fe²⁺ requires 33.9 mL of a 0.027 M KMnO₄ solution for complete reaction. What is the concentration of the Fe²⁺ in the original solution?

Question

Quizplus · Accepted Answer

The balanced equation is:MnO₄^- + 5Fe²⁺ + 8H⁺ → 5Fe³⁺ + Mn²⁺ + 4H₂OFrom the stoichiometry of the balanced equation, we can see that 1 mole of MnO₄^- reacts with 5 moles of Fe²⁺. Therefore, the concentration of Fe²⁺ in the original solution can be calculated as follows:[Fe²⁺] = (33.9 mL * 0.027 M) / (45.6 mL * 5) = 3.6 × 10^-2 M

The Ion MnO4- Is Often Used to Analyze for the Fe2+

The Ion MnO₄^- Is Often Used to Analyze for the Fe²⁺