In the reaction 2MnO₄^- + 5H₂O₂ + 6H⁺ $\rightarrow$ 2Mn²⁺ + 8H₂O + 5O₂
What volume of 0.150 M KMnO₄ solution is needed to titrate 75.0 mL of a 0.150 M H₂O₂ solution?

Question

In the reaction 2MnO₄^- + 5H₂O₂ + 6H⁺ $\rightarrow$ 2Mn²⁺ + 8H₂O + 5O₂ What volume of 0.150 M KMnO₄ solution is needed to titrate 75.0 mL of a 0.150 M H₂O₂ solution?

Quizplus · Accepted Answer

The stoichiometry of the reaction shows that 2 moles of MnO₄⁻ react with 5 moles of H₂O₂. Therefore, the volume of KMnO₄ needed is (75.0 mL * 0.150 M * 2/5) = 30.0 mL.

In the Reaction 2MnO4- + 5H2O2 + 6H+ →\rightarrow→ 2Mn2+ + 8H2O + 5O2 What Volume of 0

In the Reaction 2MnO₄^- + 5H₂O₂ + 6H⁺ $\rightarrow$ 2Mn²⁺ + 8H₂O + 5O₂
What Volume of 0