Chapter 24, Problem 123A

(a)

Interpretation Introduction

Interpretation: To calculate the pH for the given solution.

Concept Introduction: pH of the solution is described as the negative log of hydrogen ion concentration. It can be expressed as follows:

  $\begin{array}{l}\text{pH}=-\text{log}\left[{\text{H}}^{\text{+}}\right]\\ \text{or}\\ \text{pH}=-\text{log}\left[{\text{OH}}^{-}\right]\end{array}$

Answer to Problem 123A

The pH of the solution is $4.15$ .

Explanation of Solution

The concentration of the hydrogen ion is given that is $7.0\times {10}^{-5}\text{M}$ .

The pH of the solution can be calculated as follows:

  $\begin{array}{c}\text{pH}=-\text{log}\left[{\text{H}}^{\text{+}}\right]\\ =-\log \left[7.0\times {10}^{-5}\right]\\ =-\left(-4.15490\right)\\ =4.15\end{array}$

Thus, the pH of the solution is $4.15$ .

(b)

Interpretation Introduction

Interpretation: To calculate the pH for the given solution.

Concept Introduction: pH of the solution is described as the negative log of hydrogen ion concentration. It can be expressed as follows:

  $\begin{array}{l}\text{pH}=-\text{log}\left[{\text{H}}^{\text{+}}\right]\\ \text{or}\\ \text{pH}=-\text{log}\left[{\text{OH}}^{-}\right]\end{array}$

Answer to Problem 123A

The pH of the solution is $8.74$ .

Explanation of Solution

The concentration of the hydroxyl ion is given that is $1.8\times {10}^{-9}\text{M}$ .

The pH of the solution can be calculated as follows:

  $\begin{array}{c}\text{pH}=-\text{log}\left[{\text{OH}}^{-}\right]\\ =-\log \left[1.8\times {10}^{-9}\right]\\ =-\left(-8.74472\right)\\ =8.74\end{array}$

Thus, the pH of the solution is $8.74$ .

(c)

Interpretation Introduction

Interpretation: To calculate the pH for the given solution.

Concept Introduction: pH of the solution is described as the negative log of hydrogen ion concentration. It can be expressed as follows:

  $\begin{array}{l}\text{pH}=-\text{log}\left[{\text{H}}^{\text{+}}\right]\\ \text{or}\\ \text{pH}=-\text{log}\left[{\text{OH}}^{-}\right]\end{array}$

Answer to Problem 123A

The pH of the solution is $1.21$ .

Explanation of Solution

The concentration of the hydroxyl ion is given that is $6.1\times {10}^{-2}\text{M}$ .

The pH of the solution can be calculated as follows:

  $\begin{array}{c}\text{pH}=-\text{log}\left[{\text{OH}}^{-}\right]\\ =-\log \left[6.1\times {10}^{-2}\right]\\ =-\left(-1.21467\right)\\ =1.21\end{array}$

Thus, the pH of the solution is $1.21$ .

(d)

Interpretation Introduction

Interpretation: To calculate the pH for the given solution.

Concept Introduction: pH of the solution is described as the negative log of hydrogen ion concentration. It can be expressed as follows:

  $\begin{array}{l}\text{pH}=-\text{log}\left[{\text{H}}^{\text{+}}\right]\\ \text{or}\\ \text{pH}=-\text{log}\left[{\text{OH}}^{-}\right]\end{array}$

Answer to Problem 123A

The pH of the solution is $10.35$ .

Explanation of Solution

The concentration of the hydrogen ion is given that is $4.4\times {10}^{-11}\text{M}$ .

The pH of the solution can be calculated as follows:

  $\begin{array}{c}\text{pH}=-\text{log}\left[{\text{H}}^{+}\right]\\ =-\log \left[4.4\times {10}^{-11}\right]\\ =-\left(-10.35654\right)\\ =10.35\end{array}$

Thus, the pH of the solution is $10.35$ .