Chapter 16, Problem 104AP

Interpretation Introduction

(a)

Interpretation:

The hydrogen ion concentration and pH of given solutions of strong acids should be calculated.

Concept Introduction:

The concentration of hydrogen ions in a solution determines the acidity of a solution. If concentration of hydrogen ion is more than the solution is more acetic, if it is low, solution is less acidic.

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

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

Here, $\left[{\text{H}}^{+}\right]$ is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

$\text{p}\text{O}\text{H}=-\text{log}\left[{\text{OH}}^{-}\right]$

Here, $\left[{\text{OH}}^{-}\right]$ is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

$\text{p}\text{H}+\text{p}\text{O}\text{H}=14$.

Answer to Problem 104AP

The hydrogen ion concentration is $1.4\times {10}^{-3}\text{ M}$ and pH of solution is 2.85.

Explanation of Solution

Given Information:

The concentration of strong acid, ${\text{HClO}}_{\text{4}}$ is $1.4\times {10}^{-3}\text{ M}$.

Calculation:

The dissociation reaction of the acid is as follows:

${\text{HClO}}_{\text{4}}\to {\text{H}}^{+}+{\text{ClO}}_{\text{4}}{}^{-}$

Thus, if the concentration of ${\text{HClO}}_{\text{4}}$ is $1.4\times {10}^{-3}\text{ M}$ thus, hydrogen ion concentration will be $1.4\times {10}^{-3}\text{ M}$.

From the hydrogen ion concentration, pH can be calculated as follows:

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

Putting the value,

$\begin{array}{c}\text{p}\text{H}=-\text{log}\left(1.4\times {10}^{-3}\right)\\ =2.85\end{array}$

Thus, the hydrogen ion concentration is $1.4\times {10}^{-3}\text{ M}$ and pH of solution is 2.85.

Interpretation Introduction

(b)

Interpretation:

The hydrogen ion concentration and pH of given solutions of strong acids should be calculated.

Concept Introduction:

The concentration of hydrogen ions in a solution determines the acidity of a solution. If concentration of hydrogen ion is more than the solution is more acetic, if it is low, solution is less acidic.

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

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

Here, $\left[{\text{H}}^{+}\right]$ is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

$\text{p}\text{O}\text{H}=-\text{log}\left[{\text{OH}}^{-}\right]$

Here, $\left[{\text{OH}}^{-}\right]$ is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

$\text{p}\text{H}+\text{p}\text{O}\text{H}=14$.

Answer to Problem 104AP

The hydrogen ion concentration is $1.4\times {10}^{-3}\text{ M}$ and pH of solution is 2.85.

Explanation of Solution

Given Information:

The concentration of strong acid, $\text{HCl}$ is $3.0\times {10}^{-5}\text{ M}$.

Calculation:

The dissociation reaction of the acid is as follows:

$\text{HCl}\to {\text{H}}^{\text{+}}{\text{+Cl}}^{\text{-}}$

Thus, if the concentration of HCl is $3.0\times {10}^{-5}\text{ M}$ thus, hydrogen ion concentration will be $3.0\times {10}^{-5}\text{ M}$.

From the hydrogen ion concentration, pH can be calculated as follows:

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

Putting the value,

$\begin{array}{c}\text{p}\text{H}=-\text{log}\left(3.0\times {10}^{-5}\right)\\ =4.52\end{array}$

Thus, the hydrogen ion concentration is $3.0\times {10}^{-5}\text{ M}$ and pH of solution is 4.52.

Interpretation Introduction

(c)

Interpretation:

The hydrogen ion concentration and pH of given solutions of strong acids should be calculated.

Concept Introduction:

The concentration of hydrogen ions in a solution determines the acidity of a solution. If concentration of hydrogen ion is more than the solution is more acetic, if it is low, solution is less acidic.

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

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

Here, $\left[{\text{H}}^{+}\right]$ is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

$\text{p}\text{O}\text{H}=-\text{log}\left[{\text{OH}}^{-}\right]$

Here, $\left[{\text{OH}}^{-}\right]$ is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

$\text{p}\text{H}+\text{p}\text{O}\text{H}=14$.

Answer to Problem 104AP

The hydrogen ion concentration is $5.0\times {10}^{-2}\text{ M}$ and pH of solution is 1.30.

Explanation of Solution

Given Information:

The concentration of strong acid, ${\text{HNO}}_3$ is $5.0\times {10}^{-2}\text{ M}$.

Calculation:

The dissociation reaction of the acid is as follows:

${\text{HNO}}_3\to {\text{H}}^{\text{+}}{\text{+NO}}_3{}^{\text{-}}$

Thus, if the concentration of ${\text{HNO}}_3$ is $5.0\times {10}^{-2}\text{ M}$ thus, hydrogen ion concentration will be $5.0\times {10}^{-2}\text{ M}$.

From the hydrogen ion concentration, pH can be calculated as follows:

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

Putting the value,

$\begin{array}{c}\text{p}\text{H}=-\text{log}\left(5.0\times {10}^{-2}\right)\\ =1.30\end{array}$

Thus, the hydrogen ion concentration is $5.0\times {10}^{-2}\text{ M}$ and pH of solution is 1.30.

Interpretation Introduction

(d)

Interpretation:

The hydrogen ion concentration and pH of given solutions of strong acids should be calculated.

Concept Introduction:

The concentration of hydrogen ions in a solution determines the acidity of a solution. If concentration of hydrogen ion is more than the solution is more acetic, if it is low, solution is less acidic.

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

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

Here, $\left[{\text{H}}^{+}\right]$ is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

$\text{p}\text{O}\text{H}=-\text{log}\left[{\text{OH}}^{-}\right]$

Here, $\left[{\text{OH}}^{-}\right]$ is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

$\text{p}\text{H}+\text{p}\text{O}\text{H}=14$.

Answer to Problem 104AP

The hydrogen ion concentration is $5.0\times {10}^{-2}\text{ M}$ and pH of solution is 1.30.

Explanation of Solution

Given Information:

The concentration of strong acid, $\text{HCl}$ is $0.0010\text{ M}$.

Calculation:

The dissociation reaction of the acid is as follows:

$\text{HCl}\to {\text{H}}^{\text{+}}{\text{+Cl}}^{\text{-}}$

Thus, if the concentration of HCl is $0.0010\text{ M}$ thus, hydrogen ion concentration will be $0.0010\text{ M}$.

From the hydrogen ion concentration, pH can be calculated as follows:

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

Putting the value,

$\begin{array}{c}\text{p}\text{H}=-\text{log}\left(0.0010\right)\\ =3\end{array}$

Thus, the hydrogen ion concentration is $0.0010\text{ M}$ and pH of solution is 3.