Chapter 2, Problem 4P

(a)

Summary Introduction

To determine: The $\text{pH}$ of a solution having ${\text{H}}^{+}$ concentration $\left(1.75\times {10}^{-5}\text{ mol}/\text{L}\right)$.

Introduction:

The splitting of water results in the formation of two ionic species hydrogen ion and hydroxide ion. The hydrogen ions and hydroxide ions are released in equal number when the water is dissociated. The alkalinity or acidity of the solution is determined by the $\text{pH}$ (potential of hydrogen) of a solution. The negative logarithm of the molar ion hydrogen (H⁺) ion concentration is called pH. It is calculated by the formula $\text{pH}=-{\text{log [H}}^{+}\text{]}$.

Explanation of Solution

Explanation:

The given solution has $\left[{\text{H}}^{+}\right]=1.75\times {10}^{-5}\text{ mol}/\text{L}$

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

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

Substitute the values of $\left[{\text{H}}^{+}\right]$ in the above expression:

$\begin{array}{c}\text{pH}=-\log \left[{\text{H}}^{+}\right]\\ =-\log \left(1.75\times {10}^{-5}\text{ mol}/\text{L}\right)\\ =\text{4}\text{.76 }\end{array}$

Therefore, the $\text{pH}$ of the solution is $\text{4}\text{.76 }$.

Conclusion

Conclusion:

The $\text{pH}$ of solution having ${\text{H}}^{+}$ concentration ( $1.75\times {10}^{-5}\text{ mol}/\text{L}$) is $\underset{\_}{4.76}.$

(b)

Summary Introduction

To determine: The $\text{pH}$ of a solution having ${\text{H}}^{+}$ concentration $\left(\text{6}\text{.50}\times {10}^{-10}\text{ mol}/\text{L}\right)$.

Introduction:

The splitting of water results in the formation of two ionic species hydrogen ion and hydroxide ion. The hydrogen ions and hydroxide ions are released in equal number when the water is dissociated. The hydrogen ion concentration is calculated by the given $\text{pH}$ of the solution. The $\text{pH}$ of a solution is in the range of 0 to 14.

Explanation of Solution

Explanation:

The given solution has $\left[{\text{H}}^{+}\right]=\text{6}\text{.50}\times {10}^{-10}\text{ mol}/\text{L}$

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

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

Substitute the values of $\left[{\text{H}}^{+}\right]$ in the above expression:

$\begin{array}{c}\text{pH}=-\log \left[{\text{H}}^{+}\right]\\ =-\log \left(\text{6}\text{.50}\times {10}^{-10}\text{ mol}/\text{L}\right)\\ =\text{9}\text{.19 }\end{array}$

Therefore, the $\text{pH}$ of the solution is $\text{9}\text{.19 }$.

Conclusion

Conclusion:

The $\text{pH}$ of solution having ${\text{H}}^{+}$ concentration ( $\text{6}\text{.50}\times {10}^{-10}\text{ mol}/\text{L}$) is $\underset{\_}{9.19}.$

(c)

Summary Introduction

To determine: The $\text{pH}$ of a solution having ${\text{H}}^{+}$ concentration $\left(1.00\times {10}^{-4}\text{ mol}/\text{L}\right)$.

Introduction:

The splitting of water results in the formation of two ionic species hydrogen ion and hydroxide ion. The hydrogen ions and hydroxide ions are released in equal number when the water is dissociated. The alkalinity or acidity of the solution is determined by the $\text{pH}$ (potential of hydrogen) of a solution. The negative logarithm of the molar ion hydrogen (H⁺) ion concentration is called pH. It is calculated by the formula $\text{pH}=-{\text{log [H}}^{+}\text{]}$. The hydrogen ion concentration is calculated by the given $\text{pH}$ of the solution. The $\text{pH}$ of a solution is in the range of 0 to 14.

Explanation of Solution

Explanation:

The given solution has $\left[{\text{H}}^{+}\right]=1.00\times {10}^{-4}\text{ mol}/\text{L}$

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

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

Substitute the values of $\left[{\text{H}}^{+}\right]$ in the above expression:

$\begin{array}{c}\text{pH}=-\log \left[{\text{H}}^{+}\right]\\ =-\log \left(1.00\times {10}^{-4}\text{ mol}/\text{L}\right)\\ =\text{4}\text{.00}\end{array}$

Therefore, the $\text{pH}$ of the solution is $4.00$.

Conclusion

Conclusion:

The $\text{pH}$ of solution having ${\text{H}}^{+}$ concentration ( $1.00\times {10}^{-4}\text{ mol}/\text{L}$) is $\underset{\_}{4.00}.$

(d)

Summary Introduction

To determine: The $\text{pH}$ of a solution having ${\text{H}}^{+}$ concentration $\left(1.50\times {10}^{-5}\text{ mol}/\text{L}\right)$.

Introduction:

The $\text{pH}$ of a solution is defined as the negative logarithm of the molar ion hydrogen (H⁺) ion concentration. It is calculated by the formula $\text{pH}=-{\text{log [H}}^{+}\text{]}$. The hydrogen ion concentration is calculated by the given $\text{pH}$ of the solution. The $\text{pH}$ of a solution is in the range of 0 to 14.

Explanation of Solution

Explanation:

The given solution has $\left[{\text{H}}^{+}\right]=1.50\times {10}^{-5}\text{ mol}/\text{L}$

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

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

Substitute the values of $\left[{\text{H}}^{+}\right]$ in the above expression:

$\begin{array}{c}\text{pH}=-\log \left[{\text{H}}^{+}\right]\\ =-\log \left(1.50\times {10}^{-5}\text{ mol}/\text{L}\right)\\ =\text{4}\text{.82}\end{array}$

Therefore, the $\text{pH}$ of the solution is $\text{4}\text{.76 }$.

Conclusion

Conclusion:

The $\text{pH}$ of solution having ${\text{H}}^{+}$ concentration ( $1.50\times {10}^{-5}\text{ mol}/\text{L}$) is $\underset{\_}{4.82}.$