Under basic conditions, the correctly balanced redox reaction for
PO₃^3-(aq) + MnO₄^-(aq) $\rarr$ PO₄^3-(aq) + MnO₂(s) is:
3PO₃^3-(aq) + 2MnO₄^-(aq) + H₂O(l) $\rarr$ 3PO₄^3-(aq) + 2MnO₂(s) + 2OH^-(aq)

Question

Under basic conditions, the correctly balanced redox reaction for
PO₃^3-(aq) + MnO₄^-(aq)

\rarr

PO₄^3-(aq) + MnO₂(s) is:
3PO₃^3-(aq) + 2MnO₄^-(aq) + H₂O(l)

\rarr

3PO₄^3-(aq) + 2MnO₂(s) + 2OH^-(aq)

Quizplus · Accepted Answer

The coefficients in the balanced equation indicate that three molecules of the sulfite ion and two molecules of the permanganate ion react with one molecule of the dioxide ion and two molecules of the hydroxide ion to form three molecules of the sulfate ion and two solid manganese(II) oxide molecules, with two molecules of water as a byproduct. This equation represents a redox reaction, with the manganese(II) oxide serving as the oxidizing agent and the sulfite ion serving as the reducing agent.

Under Basic Conditions, the Correctly Balanced Redox Reaction for PO33-(aq) →\rarr→

Under Basic Conditions, the Correctly Balanced Redox Reaction for
PO₃^3-(aq) $\rarr$