Chapter 7, Problem 7.132MP

(a)

Interpretation Introduction

Interpretation:

Balanced net ionic equation for the reaction has to be determined.

Concept introduction:

Net ionic equation is used to show only the chemicals and ions involved in a chemical reaction in order to simply the information about the reaction.

Steps involved in balancing the net ionic equation is

Step.1- Write the unbalanced net ionic equation.

Step.2- Decide which atoms are oxidized and which are reduced and write the two unbalanced half-reactions.

Step 3- Balance both half-reactions for all atoms except $O$ and $H$.

Step 4- Balance each half reaction for $O$ by adding water to the side with less $O$ and balance for $H$ by adding $H^{+}$ to each side with less $H$

Step 5- Balance each half-reactions for charge by adding the electrons to the side with greater positive charge and then multiply by suitable factors to make the electron count the same in both half-reactions.

Step 6- Add the two balanced half-reactions together and cancel electrons and other species that appear on the sides of the equation.

(b)

Interpretation Introduction

Interpretation:

Concentration of all the ions in the solution after reaction to make it electrically neutral has to be calculated.

Concept Introduction:

Molarity $\left(\text{M}\right)$ is the ratio of number of moles of solute to volume in liters is given by

$\text{Molarity=}\frac{\text{Moles}\text{of}\text{solute}}{\text{Liters}\text{of}\text{solution}}$

So, $Molesofsolute=Molarity\times Litersofsolution$

Concentration of ion is the ionic strength in the solution when dissolved in water.