$$ \ce{5H2O2(aq) + 2MnO4-(aq) + 6H+(aq) -> 2Mn^{2+}(aq) + 8H2O(l) +5O2(g)} $$

In a titration experiment, \(\ce{H2O2(aq)}\) reacts with aqueous \(\ce{MnO4-(aq)}\) as represented by the equation above.

Which element is being oxidized during the titration, and what is the element's change in oxidation number?

Summary Submit

Although oxygen typically has an oxidation state of -2 in compounds, it is -1 in hydrogen peroxide \(\ce{H2O2}\). The oxidation state for oxygen in diatomic oxygen is 0.

The oxidation state of manganese changes from +7 to +2, but this is reduction (gain of electrons).