Chapter 17, Problem 51CE

Interpretation Introduction

Interpretation:

Balanced equation of reaction below if concentration of hydroxide ion is $\text{3}\text{.4}\times {\text{10}}^{-10}M$ has to be determined.

  ${\text{Fe}}^{2+}\left(aq\right)+{\text{MnO}}_4^{-}\left(aq\right)\to {\text{Fe}}^{3+}\left(aq\right)+{\text{Mn}}^{2+}\left(aq\right)$

Concept Introduction:

Rules to balance redox reactions by ion-electron method are as follows:

1. Two half-reactions with elements that got oxidized and reduced should be written.

2. Elements other than oxygen and hydrogen should be balanced.

3. Conditions to balance $\text{O}$ and $\text{H}$ are as follows:

In acidic solution, ${\text{H}}^{+}$ and ${\text{H}}_2\text{O}$ should be used to balance $\text{O}$ and $\text{H}$.

In basic solution, equal ${\text{OH}}^{-}$ ions to ${\text{H}}^{+}$ ions should be added on both sides of balanced reaction in acidic medium.

4. For acidic medium, charge is balanced by addition of ${\text{H}}^{+}$ ion. Then combine ${\text{H}}^{+}$ and ${\text{OH}}^{-}$ to form ${\text{H}}_2\text{O}$ and cancel common ${\text{H}}_2\text{O}$ in reaction.

5. Electrons should be added to balance electric charge.

6. Finally, two half-reactions should be added and any common substance including electrons must be cancelled.