Chapter 16, Problem 70E

Interpretation Introduction

Interpretation:

Each redox reaction occurring in basic solution is to be balanced.

Concept Introduction: Oxidation is defined as the loss of electrons.

Reduction is defined as the gain of electrons.

When oxidation and reduction simultaneously take place, then it is known as redox reaction.

In balanced redox reaction, each of the atom on both sides of reactions is equal.

To balance the redox reaction, follow the following steps:

Assign the oxidation states to all the atoms. Identify the substances that are being oxidized and reduced.

Separate the reaction into two half-reactions: oxidation half reaction and reduction half reaction.

Balance each of the half-reaction with respect to mass in the following order:

Balance all the elements other than $H$ and $O$ elements.

Balance $O$ element by adding $H_{2}O$.

Balance $H$ element by adding $H^{+}$.

Balance the charges

Balance each of the half-reaction with respect to charge by adding the electrons to the right side of the oxidation half-reaction and the left side of the reduction half-reaction.

Multiply one or both half-reactions (if required) by a small whole-number so as to make sure the number of electrons in both half-reactions by a small whole number.

Add the two half reactions by cancelling electrons and other species (if required) to obtain a balanced chemical reaction.

Verify that the reaction is balanced with respect to both mass and charge.