Chemistry - Complete d-block Question with Solution | TestHub

This ${\mathrm{KMnO}}_4$ is a powerful oxidizing agent in neutral, acidic, and alkaline medium. The ${\mathrm{H}}_2{\mathrm{O}}_2$ is also an oxidizing agent but in the reaction of ${\mathrm{KMnO}}_4$ with the ${\mathrm{H}}_2{\mathrm{O}}_2$. The ${\mathrm{H}}_2{\mathrm{O}}_2$loses its electron and acts as a reducing agent. In an acidic medium, the${\mathrm{MnO}}_4^{-}$ ions involve the addition of 5 electrons and the two peroxide ions give out two electrons. In dilute alkaline medium or in neutral medium ${\mathrm{MnO}}_4^{-}$ ions involve the addition of 3 electrons. The reaction in basic medium is given below.

$2{\mathrm{KMnO}}_4+3{\mathrm{H}}_2{\mathrm{O}}_2\stackrel{\mathrm{basic} \mathrm{medium}}{⟶}\stackrel{+4}{2{\mathrm{MnO}}_2}+3{\mathrm{O}}_2+2{\mathrm{H}}_2\mathrm{O}+2\mathrm{KOH}$

The oxidation state of $\mathrm{Mn} \text{in} {\mathrm{MnO}}_2$ is $+4.$