Chapter 16, Problem 16.31QP

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

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

Answer to Problem 16.31QP

The value of $\text{pH}$ is $\underset{\_}{7.46}$ and the value of $\text{pOH}$ is $\underset{\_}{6.54}$ for the given solution. The solution is basic in nature.

Explanation of Solution

Given

The concentration of hydrogen ion ${\text{H}}^{+}$ is $3.48\times {10}^{-8}\text{M}$.

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.

$\begin{array}{c}\text{pH}=-\log \left(3.48\times {10}^{-8}\right)\\ =-\left(7.46\right)\\ =\underset{\_}{7.46}\end{array}$

Therefore, the value of $\text{pH}$ is $\underset{\_}{7.46}$ 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.

$\begin{array}{c}\text{pOH}=14-7.46\\ =\underset{\_}{6.54}\end{array}$

Therefore, the value of $\text{pOH}$ for the given solution is $\underset{\_}{6.54}$.

The value of $\text{pH}$ is more than $7$ so, it is a basic 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 $\text{pH}$ value of the given solution is calculated by the formula,

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

Answer to Problem 16.31QP

The value of $\text{pH}$ is $\underset{\_}{4.69}$ and the value of $\text{pOH}$ is $\underset{\_}{9.31}$ for the given solution. The solution is acidic in nature.

Explanation of Solution

Given

The concentration of hydrogen ion ${\text{H}}^{+}$ is $2.0\times {10}^{-5}\text{M}$.

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.

$\begin{array}{c}\text{pH}=-\log \left(2.0\times {10}^{-5}\right)\\ =-\left(-4.69\right)\\ =\underset{\_}{4.69}\end{array}$

Therefore, the value of $\text{pH}$ is $\underset{\_}{4.69}$ 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.

$\begin{array}{c}\text{pOH}=14-4.69\\ =\underset{\_}{9.31}\end{array}$

Therefore, the value of $\text{pOH}$ for the given solution is $\underset{\_}{9.31}$.

The value of $\text{pH}$ is less than $7$ so, it is an acidic 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 16.31QP

The value of $\text{pH}$ is $\underset{\_}{7.15}$ and the value of $\text{pOH}$ is $\underset{\_}{6.85}$ for the given solution. The solution is basic in nature.

Explanation of Solution

Given

The concentration of hydrogen ion ${\text{H}}^{+}$ is $7.0\times {10}^{-8}\text{M}$.

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.

$\begin{array}{c}\text{pH}=-\log \left(7.0\times {10}^{-8}\right)\\ =-\left(-7.15\right)\\ =\underset{\_}{7.15}\end{array}$

Therefore, the value of $\text{pH}$ is $\underset{\_}{7.15}$ 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.

$\begin{array}{c}\text{pOH}=14-7.15\\ =\underset{\_}{6.85}\end{array}$

Therefore, the value of $\text{pOH}$ for the given solution is $\underset{\_}{6.85}$.

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

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

Answer to Problem 16.31QP

The value of $\text{pH}$ is $\underset{\_}{10.94}$ and the value of $\text{pOH}$ is $\underset{\_}{3.06}$ for the given solution. The solution is basic in nature.

Explanation of Solution

Given

The concentration of hydroxide ion ${\text{OH}}^{-}$ is $8.56\times {10}^{-4}\text{M}$.

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.

$\begin{array}{c}\text{pOH}=-\log \left(8.56\times {10}^{-4}\right)\\ =-\left(-3.06\right)\\ =\underset{\_}{3.06}\end{array}$

Therefore, the value of $\text{pOH}$ is $\underset{\_}{3.06}$ 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.

$\begin{array}{c}\text{pH}=14-3.06\\ =\underset{\_}{10.94}\end{array}$

Therefore, the value of $\text{pH}$ for the given solution is $\underset{\_}{10.94}$.

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

Conclusion

1. a. The value of $\text{pH}$ is $\underset{\_}{7.46}$ and the value of $\text{pOH}$ is $\underset{\_}{6.54}$ for the given solution. The solution is basic in nature.
2. b. The value of $\text{pH}$ is $\underset{\_}{4.69}$ and the value of $\text{pOH}$ is $\underset{\_}{9.31}$ for the given solution. The solution is acidic in nature.
3. c. The value of $\text{pH}$ is $\underset{\_}{7.15}$ and the value of $\text{pOH}$ is $\underset{\_}{6.85}$ for the given solution. The solution is basic in nature.
4. d. The value of $\text{pH}$ is $\underset{\_}{10.94}$ and the value of $\text{pOH}$ is $\underset{\_}{3.06}$ for the given solution. The solution is basic in nature.