Chapter 16, Problem 41A

(a)

Interpretation Introduction

Interpretation:

The concentration of H+ ion and the pH of the solutions have to be calculated.

Concept Introduction:

For all strong monobasic acids, the concentration of the acid is the concentration of ${\mathrm{H}}^{+}$ ions.

For strong dibasic acid, the concentration of ${\mathrm{H}}^{+}$ ions are twice than the concentration of the acid.

The acidity or alkalinity of a solution is expressed by determining pH of the solution. pH of a solution is defined as negative logarithm of the concentration of ${\mathrm{H}}^{+}$ ion in the solution. pH is expressed as-

  $\text{pH}=-\mathrm{l}\mathrm{o}\mathrm{g}[{\mathrm{H}}^{+}]$

Answer to Problem 41A

[ ${\mathrm{H}}^{+}$ ] in H₂SO₄ solution is 3.0 M and pH of H₂SO₄ solution is -0.477.

Explanation of Solution

For all strong monobasic acids, the concentration of the acid is the concentration of ${\mathrm{H}}^{+}$ ions.

For strong dibasic acid, the concentration of ${\mathrm{H}}^{+}$ ions is twice than the concentration of the acid.

Concentration of H₂SO₄ solution = 1.50 M

[ ${\mathrm{H}}^{+}$ ] in H₂SO₄ solution will be $2\times 1.50\text{ M = 3}\text{.00 M}$ as H₂SO₄ gives 2 ${\mathrm{H}}^{+}$ ions in the solution.

  $\begin{array}{l}\text{pH}=-\mathrm{l}\mathrm{o}\mathrm{g}[{\mathrm{H}}^{+}]\\ =-\mathrm{l}\mathrm{o}\mathrm{g}[3.0]\\ =-0.477\end{array}$

Thus, pH of H₂SO₄ solution is -0.477.

(b)

Interpretation Introduction

Interpretation:

The concentration of H+ ion and the pH of the solutions have to be calculated.

Concept Introduction:

For all strong monobasic acids, the concentration of the acid is the concentration of ${\mathrm{H}}^{+}$ ions.

For strong dibasic acid, the concentration of ${\mathrm{H}}^{+}$ ions are twice than the concentration of the acid.

The acidity or alkalinity of a solution is expressed by determining pH of the solution. pH of a solution is defined as negative logarithm of the concentration of ${\mathrm{H}}^{+}$ ion in the solution. pH is expressed as-

  $\text{pH}=-\mathrm{l}\mathrm{o}\mathrm{g}[{\mathrm{H}}^{+}]$

Answer to Problem 41A

[H⁺] in HBr solution is 9.47 × 10-4 M and P^H of HBr solution is 3.02.

Explanation of Solution

For all strong monobasic acids, the concentration of the acid is the concentration of ${\text{H}}^{+}$ ions.

For strong dibasic acid, the concentration of ${\text{H}}^{+}$ ions is twice than the concentration of the acid.

Concentration of HBr solution = 9.47 × 10-4 M

[ ${\text{H}}^{+}$ ] in HBr solution = 9.47 × 10-4 M

  $\begin{array}{l}\text{pH}=-\mathrm{l}\mathrm{o}\mathrm{g}[{\mathrm{H}}^{+}]\\ =-\mathrm{l}\mathrm{o}\mathrm{g}[9.47\times \mathrm{}10^{-4}]\\ =3.02\end{array}$

Thus, pH of HBr solution is 3.02.

(c)

Interpretation Introduction

Interpretation:

The concentration of H+ ion and the pH of the solutions have to be calculated.

Concept Introduction:

For all strong monobasic acids, the concentration of the acid is the concentration of ${\mathrm{H}}^{+}$ ions.

For strong dibasic acid, the concentration of ${\mathrm{H}}^{+}$ ions are twice than the concentration of the acid.

The acidity or alkalinity of a solution is expressed by determining pH of the solution. pH of a solution is defined as negative logarithm of the concentration of ${\mathrm{H}}^{+}$ ion in the solution. pH is expressed as-

  $\text{pH}=-\mathrm{l}\mathrm{o}\mathrm{g}[{\mathrm{H}}^{+}]$

Answer to Problem 41A

Concentration of ${\text{H}}^{+}$ in HNO₃ solutionis1.63 × 10-3 M and pH of HNO₃ solution is 2.79.

Explanation of Solution

For all strong monobasic acids, the concentration of the acid is the concentration of ${\text{H}}^{+}$ ions.

For strong dibasic acid, the concentration of ${\text{H}}^{+}$ ions is twice than the concentration of the acid.

Concentration of HNO₃ solution = 1.63× 10-3 M

[H⁺] in HNO₃ solution = 1.63 × 10-³M

  $\begin{array}{l}{\mathrm{P}}^{\mathrm{H}}=-\mathrm{l}\mathrm{o}\mathrm{g}[{\mathrm{H}}^{+}]\\ =-\mathrm{l}\mathrm{o}\mathrm{g}[1.63\times \mathrm{}10^{-3}]\\ =2.79\end{array}$

Thus, pH of HNO₃ solution is 2.79.

(d)

Interpretation Introduction

Interpretation:

The concentration of H+ ion and the pH of the solutions have to be calculated.

Concept Introduction:

For all strong monobasic acids, the concentration of the acid is the concentration of ${\mathrm{H}}^{+}$ ions.

For strong dibasic acid, the concentration of ${\mathrm{H}}^{+}$ ions are twice than the concentration of the acid.

The acidity or alkalinity of a solution is expressed by determining pH of the solution. pH of a solution is defined as negative logarithm of the concentration of ${\mathrm{H}}^{+}$ ion in the solution. pH is expressed as-

  $\text{pH}=-\mathrm{l}\mathrm{o}\mathrm{g}[{\mathrm{H}}^{+}]$

Answer to Problem 41A

[ ${\text{H}}^{+}$ ] in HCl solutionis5.58 × 10-2 M and P^H of HCl solution is 1.25.

Explanation of Solution

For all strong monobasic acids, the concentration of the acid is the concentration of ${\text{H}}^{+}$ ions.

For strong dibasic acid, the concentration of ${\text{H}}^{+}$ ions is twice than the concentration of the acid.

Concentration of HCl solution = 5.58× 10-2 M

[ ${\text{H}}^{+}$ ] in HCl solution = 5.58 × 10-2 M

  $\begin{array}{l}\text{pH}=-\mathrm{l}\mathrm{o}\mathrm{g}[{\mathrm{H}}^{+}]\\ =-\mathrm{l}\mathrm{o}\mathrm{g}[5.58\times \mathrm{}10^{-2}]\\ =1.25\end{array}$

The pH of HCl solution is 1.25.