Chapter 16, Problem 16.32QP

(a)

Interpretation Introduction

To determine: The value of $\text{pH}$ and $\text{pOH}$ of the solution from the given hydrogen ion concentration and if the given solution is acidic, basic or neutral.

Interpretation: The value of $\text{pH}$ and $\text{pOH}$ of the solution from the given hydrogen concentration are to be calculated. The solution being acidic, basic or neutral is to be indicated.

Concept introduction: The $\text{pH}$ value determines if a given solution is acidic, basic and neutral in nature.

The $\text{pOH}$ value of the given solution is calculated by the formula,

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

Answer to Problem 16.32QP

The value of $\text{pH}$ is $\underset{\_}{4.16}$ and the value of $\text{pOH}$ is $\underset{\_}{9.84}$ for the given solution. The solution is acidic in nature.

Explanation of Solution

Given

The concentration of hydroxide ion ${\text{OH}}^{-}$ is $1.44\times {10}^{-10}\text{M}$.

The $\text{pOH}$ value of the given solution is calculated by the formula,

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

Substitute the concentration of ${\text{OH}}^{-}$ in the above expression.

$\begin{array}{c}\text{pOH}=-\log \left(1.44\times {10}^{-10}\right)\\ =-\left(-9.84\right)\\ =\underset{\_}{9.84}\end{array}$

Therefore, the value of $\text{pOH}$ is $\underset{\_}{9.84}$ of the given solution.

The value of $\text{pH}$ of the given solution is calculated by the formula,

$\text{pH}+\text{pOH}=14$

Substitute value of $\text{pOH}$ in the above expression.

$\begin{array}{c}\text{pH}=14-9.84\\ =\underset{\_}{4.16}\end{array}$

Therefore, the value of $\text{pH}$ for the given solution is $\underset{\_}{4.16}$.

The value of $\text{pH}$ is less than $7$ so, it is an acidic solution.

(b)

Interpretation Introduction

To determine: The value of $\text{pH}$ and $\text{pOH}$ of the solution from the given hydrogen ion concentration and if the given solution is acidic, basic or neutral.

Interpretation: The value of $\text{pH}$ and $\text{pOH}$ of the solution from the given hydrogen concentration are to be calculated. The solution being acidic, basic or neutral is to be indicated.

Concept introduction: The $\text{pH}$ value determines if a given solution is acidic, basic and neutral in nature.

The $\text{pOH}$ value of the given solution is calculated by the formula,

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

Answer to Problem 16.32QP

The value of $\text{pH}$ is $\underset{\_}{12.81}$ and the value of $\text{pOH}$ is $\underset{\_}{1.19}$ for the given solution. The solution is basic in nature.

Explanation of Solution

Given

The concentration of hydroxide ion ${\text{OH}}^{-}$ is $6.37\times {10}^{-2}\text{M}$.

The $\text{pOH}$ value of the given solution is calculated by the formula,

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

Substitute the concentration of ${\text{OH}}^{-}$ in the above expression.

$\begin{array}{c}\text{pOH}=-\log \left(6.37\times {10}^{-2}\right)\\ =-\left(-1.19\right)\\ =\underset{\_}{1.19}\end{array}$

Therefore, the value of $\text{pOH}$ is $\underset{\_}{1.19}$ of the given solution.

The value of $\text{pH}$ of the given solution is calculated by the formula,

$\text{pH}+\text{pOH}=14$

Substitute value of $\text{pH}$ in the above expression.

$\begin{array}{c}\text{pH}=14-1.19\\ =\underset{\_}{12.81}\end{array}$

Therefore, the value of $\text{pH}$ for the given solution is $\underset{\_}{12.81}$.

The value of $\text{pH}$ is more than $7$ so, it is a basic solution.

(c)

Interpretation Introduction

To determine: The value of $\text{pH}$ and $\text{pOH}$ of the solution from the given hydrogen ion concentration and if the given solution is acidic, basic or neutral.

Interpretation: The value of $\text{pH}$ and $\text{pOH}$ of the solution from the given hydrogen concentration are to be calculated. The solution being acidic, basic or neutral is to be indicated.

Concept introduction: The $\text{pH}$ value determines if a given solution is acidic, basic and neutral in nature.

The $\text{pH}$ value of the given solution is calculated by the formula,

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

Answer to Problem 16.32QP

The value of $\text{pH}$ is $\underset{\_}{8.48}$ and the value of $\text{pOH}$ is $\underset{\_}{5.52}$ for the given solution. The solution is basic in nature.

Explanation of Solution

Given

The given concentration of hydrogen ion ${\text{H}}^{+}$ is $3.39\times {10}^{-9}\text{M}$.

The $\text{pH}$ value of the given solution is calculated by the formula,

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

Substitute the concentration of ${\text{H}}^{+}$ in the above expression.

$\begin{array}{c}\text{pH}=-\log \left(3.39\times {10}^{-9}\right)\\ =-\left(-8.48\right)\\ =\underset{\_}{8.48}\end{array}$

Therefore, the value of $\text{pH}$ is $\underset{\_}{8.48}$ of the given solution.

The value of $\text{pOH}$ of the given solution is calculated by the formula,

$\text{pH}+\text{pOH}=14$

Substitute value of $\text{pH}$ in the above expression.

$\begin{array}{c}\text{pOH}=14-8.48\\ =\underset{\_}{5.52}\end{array}$

Therefore, the value of $\text{pOH}$ for the given solution is $\underset{\_}{5.52}$.

The value of $\text{pH}$ is more than $7$ so, it is a basic solution.

(d)

Interpretation Introduction

To determine: The value of $\text{pH}$ and $\text{pOH}$ of the solution from the given hydrogen ion concentration and if the given solution is acidic, basic or neutral.

Interpretation: The value of $\text{pH}$ and $\text{pOH}$ of the solution from the given hydrogen concentration are to be calculated. The solution being acidic, basic or neutral is to be indicated.

Concept introduction: The $\text{pH}$ value determines if a given solution is acidic, basic and neutral in nature.

The $\text{pH}$ value of the given solution is calculated by the formula,

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

Answer to Problem 16.32QP

The value of $\text{pH}$ is $\underset{\_}{2.30}$ and the value of $\text{pOH}$ is $\underset{\_}{11.7}$ for the given solution. The solution is acidic in nature.

Explanation of Solution

Given information:

The concentration of hydrogen ion ${\text{H}}^{+}$ is $4.92\times {10}^{-3}\text{M}$.

The $\text{pH}$ value of the given solution is calculated by the formula,

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

Substitute the concentration of ${\text{H}}^{+}$ in the above expression.

$\begin{array}{c}\text{pH}=-\log \left(4.92\times {10}^{-3}\right)\\ =-\left(2.30\right)\\ =\underset{\_}{2.30}\end{array}$

Therefore, the value of $\text{pH}$ is $\underset{\_}{2.30}$ of the given solution.

The value of $\text{pOH}$ of the given solution is calculated by the formula,

$\text{pH}+\text{pOH}=14$

Substitute value of $\text{pH}$ in the above expression.

$\begin{array}{c}\text{pOH}=14-2.30\\ =\underset{\_}{11.7}\end{array}$

Therefore, the value of $\text{pOH}$ for the given solution is $\underset{\_}{11.7}$.

The value of $\text{pH}$ is less than $7$ so, it is an acidic solution.

Conclusion

1. a. The value of $\text{pH}$ is $\underset{\_}{4.16}$ and the value of $\text{pOH}$ is $\underset{\_}{9.84}$ for the given solution. The solution is acidic in nature.
2. b. The value of $\text{pH}$ is $\underset{\_}{12.81}$ and the value of $\text{pOH}$ is $\underset{\_}{1.19}$ for the given solution. The solution is basic in nature.
3. c. The value of $\text{pH}$ is $\underset{\_}{8.48}$ and the value of $\text{pOH}$ is $\underset{\_}{5.52}$ for the given solution. The solution is basic in nature.
4. d. The value of $\text{pH}$ is $\underset{\_}{2.30}$ and the value of $\text{pOH}$ is $\underset{\_}{11.7}$ for the given solution. The solution is acidic in nature.