Chapter 16, Problem 44QAP

Interpretation Introduction

(a)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

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:

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

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

9.69, Basic.

Given Information:

The hydroxide ion concentration is $4.85\times {10}^{-5}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(4.85\times {10}^{-5}\right)\\ =4.31\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-4.31\\ =9.69\end{array}$

Since, the pH of solution is more than 7 thus, the solution is basic in nature.

(b)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

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:

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

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

7.6, Basic.

Given Information:

The hydroxide ion concentration is $3.96\times {10}^{-7}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(3.96\times {10}^{-7}\right)\\ =6.40\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-6.40\\ =7.6\end{array}$

Since, the pH of solution is more than 7 thus, the solution is basic in nature.

(c)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

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:

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

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

4.09, Acidic.

Given Information:

The hydroxide ion concentration is $1.22\times {10}^{-10}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(1.22\times {10}^{-10}\right)\\ =9.91\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-9.91\\ =4.09\end{array}$

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

(d)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

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:

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

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

2.7, Acidic.

Given Information:

The hydroxide ion concentration is $5.33\times {10}^{-12}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(5.33\times {10}^{-12}\right)\\ =11.3\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-11.3\\ =2.7\end{array}$

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

Answer to Problem 44QAP

9.69, Basic.

Explanation of Solution

Given Information:

The hydroxide ion concentration is $4.85\times {10}^{-5}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(4.85\times {10}^{-5}\right)\\ =4.31\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-4.31\\ =9.69\end{array}$

Since, the pH of solution is more than 7 thus, the solution is basic in nature.

Interpretation Introduction

(b)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

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:

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

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

7.6, Basic.

Given Information:

The hydroxide ion concentration is $3.96\times {10}^{-7}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(3.96\times {10}^{-7}\right)\\ =6.40\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-6.40\\ =7.6\end{array}$

Since, the pH of solution is more than 7 thus, the solution is basic in nature.

(c)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

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:

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

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

4.09, Acidic.

Given Information:

The hydroxide ion concentration is $1.22\times {10}^{-10}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(1.22\times {10}^{-10}\right)\\ =9.91\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-9.91\\ =4.09\end{array}$

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

(d)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

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:

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

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

2.7, Acidic.

Given Information:

The hydroxide ion concentration is $5.33\times {10}^{-12}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(5.33\times {10}^{-12}\right)\\ =11.3\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-11.3\\ =2.7\end{array}$

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

Answer to Problem 44QAP

7.6, Basic.

Explanation of Solution

Given Information:

The hydroxide ion concentration is $3.96\times {10}^{-7}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(3.96\times {10}^{-7}\right)\\ =6.40\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-6.40\\ =7.6\end{array}$

Since, the pH of solution is more than 7 thus, the solution is basic in nature.

Interpretation Introduction

(c)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

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:

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

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

4.09, Acidic.

Given Information:

The hydroxide ion concentration is $1.22\times {10}^{-10}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(1.22\times {10}^{-10}\right)\\ =9.91\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-9.91\\ =4.09\end{array}$

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

(d)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

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:

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

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

2.7, Acidic.

Given Information:

The hydroxide ion concentration is $5.33\times {10}^{-12}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(5.33\times {10}^{-12}\right)\\ =11.3\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-11.3\\ =2.7\end{array}$

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

Answer to Problem 44QAP

4.09, Acidic.

Explanation of Solution

Given Information:

The hydroxide ion concentration is $1.22\times {10}^{-10}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(1.22\times {10}^{-10}\right)\\ =9.91\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-9.91\\ =4.09\end{array}$

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

Interpretation Introduction

(d)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

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:

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

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

2.7, Acidic.

Given Information:

The hydroxide ion concentration is $5.33\times {10}^{-12}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(5.33\times {10}^{-12}\right)\\ =11.3\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-11.3\\ =2.7\end{array}$

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

Answer to Problem 44QAP

2.7, Acidic.

Explanation of Solution

Given Information:

The hydroxide ion concentration is $5.33\times {10}^{-12}\text{ M}$

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

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

Putting the values,

$\begin{array}{c}\text{p}\text{O}\text{H}=-\text{log}\left(5.33\times {10}^{-12}\right)\\ =11.3\end{array}$

The pH of solution is calculated as follows:

$\text{p}\text{H}=14-\text{p}\text{O}\text{H}$

Putting the values,

$\begin{array}{c}\text{p}\text{H}=14-11.3\\ =2.7\end{array}$

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.