Chapter 13, Problem 91E

(a)

Interpretation Introduction

Interpretation: The major species present in $0.015\text{M}$ solutions of the following bases are to be stated. The $\left[{\text{OH}}^{-}\right]$ and the $\text{pH}$ value of the given solutions is to be calculated.

Concept introduction: The $\text{pH}$ of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution. A logarithmic scale is used on which, the value $7$ corresponds to a neutral species, a value less than $7$ corresponds to an acid and a value greater than $7$ corresponds to a base.

The $\text{pH}$ of a solution is calculated by the formula, $\text{pH}=-\log \left[{\text{H}}^{+}\right]$

The $\text{pOH}$ of a solution is calculated by the formula, $\text{pOH}=-\log \left[{\text{OH}}^{-}\right]$

The sum, $\text{pH}+\text{pOH}=14$

To determine: The major species present in $0.015\text{M}$ solution of $\text{KOH}$ and the $\left[{\text{OH}}^{-}\right]$ and the $\text{pH}$ value of this solution.

(b)

Interpretation Introduction

Interpretation: The major species present in $0.015\text{M}$ solutions of the following bases are to be stated. The $\left[{\text{OH}}^{-}\right]$ and the $\text{pH}$ value of the given solutions is to be calculated.

Concept introduction: The $\text{pH}$ of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution. A logarithmic scale is used on which, the value $7$ corresponds to a neutral species, a value less than $7$ corresponds to an acid and a value greater than $7$ corresponds to a base.

The $\text{pH}$ of a solution is calculated by the formula, $\text{pH}=-\log \left[{\text{H}}^{+}\right]$

The $\text{pOH}$ of a solution is calculated by the formula, $\text{pOH}=-\log \left[{\text{OH}}^{-}\right]$

The sum, $\text{pH}+\text{pOH}=14$

To determine: The major species present in $0.015\text{M}$ solution of $\text{Ba}{\left(\text{OH}\right)}_2$ and the $\left[{\text{OH}}^{-}\right]$ and the $\text{pH}$ value of this solution.