Chapter 14, Problem 104E

Interpretation Introduction

Interpretation:

For the given table, the missing hydrogen ion concentration $\left[{\text{H}}_3{\text{O}}^{+}\right]$, hydroxide ion concentration $\left[{\text{OH}}^{-}\right]$, pH, pOH and nature of the solution should be determined.

Concept information:

The pH of a solution is expressed by the formula as follows:

$\text{pH}=-\text{log}\left[{\text{H}}_3{\text{O}}^{+}\right]$

The $\text{pH}$ scale is used to classify the solution as follows:

The solution having pH value less than 7 is acidic.

The solution having pH value greater than 7 is basic.

If the solution has pH equal to 7, then it is neutral.

The pOH of a solution is expressed by the formula as follows:

$\text{pOH}=-\text{log}\left[{\text{OH}}^{-}\right]$

The sum of pOH and pH of a solution is equal to 14.

$\text{pOH}+\text{pH}=14.0$

The ion product constant is expressed as follows:

$\left[{\text{H}}_3{\text{O}}^{+}\right]\left[{\text{OH}}^{-}\right]=K_w=1.0\times {10}^{-14}$

The solution is acidic if the concentration of hydronium ions is less than $1.0\times {10}^{-7}\text{M}$ and vice-versa.

The solution is basic if concentration of hydroxide ions is more than $1.0\times {10}^7\text{M}$$1.0\times {10}^{-7}\text{M}$ and vice-versa.