Chapter 4, Problem 4.111QP

Interpretation Introduction

Interpretation: The redox reaction of the given equation in which soluble ${\text{Mn}}^{2+}$ becomes solid ${\text{MnO}}_{\text{2}}$ is to be completed and a balanced equation of the same is to be stated.

Concept introduction: The reaction in which reduction and oxidation process occurs simultaneously is termed as redox reaction.

In oxidation there is loss of electrons occur which increases the oxidation state of an atom whereas in reduction process there is gaining of electrons occur which decreases the oxidation state of an atom.

A reducing agent will lose electrons and will oxidize itself whereas a oxidizing agent will gain electrons and will reduce itself.

To determine:  The complete and balanced redox equation from the given reaction in which soluble ${\text{Mn}}^{2+}$ becomes solid ${\text{MnO}}_{\text{2}}$. The given reaction is,

$\text{Fe}{\left(\text{OH}\right)}_{\text{2}}{}^{+}\left(aq\right)+{\text{Mn}}^{2+}\left(aq\right)\to {\text{MnO}}_{\text{2}}\left(s\right)+{\text{Fe}}^{2+}\left(aq\right)$