Chapter 16.5, Problem 7PPB

(a)

Interpretation Introduction

Interpretation:

The pH of the given aqueous solutions at ${\text{25}}^{\circ }\text{C}$ has to be calculated

Concept Information:

Strong acids:

In strong acids, the ionization of acid is complete. This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium.

pH definition:

The concentration of hydrogen ion is measured using $\text{pH}$ scale.  The acidity of aqueous solution is expressed by $\text{pH}$ scale.

The $\text{pH}$ of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

$\text{pH}\text{=}{\text{-log[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$

On rearranging, the concentration of hydrogen ion ${\text{[H}}^{+}\text{]}$ can be calculated using pH as follows,

${\text{[H}}^{+}\text{]}\text{=}{\text{10}}^{\text{-pH}}$

To calculate: The pH of an aqueous solution of 0.011 M ${\text{HNO}}_{\text{3}}$

(b)

Interpretation Introduction

Interpretation:

The pH of the given aqueous solutions at ${\text{25}}^{\circ }\text{C}$ has to be calculated

Concept Information:

Strong acids:

In strong acids, the ionization of acid is complete. This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium.

pH definition:

The concentration of hydrogen ion is measured using $\text{pH}$ scale.  The acidity of aqueous solution is expressed by $\text{pH}$ scale.

The $\text{pH}$ of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

$\text{pH}\text{=}{\text{-log[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$

On rearranging, the concentration of hydrogen ion ${\text{[H}}^{+}\text{]}$ can be calculated using pH as follows,

${\text{[H}}^{+}\text{]}\text{=}{\text{10}}^{\text{-pH}}$

To calculate: The pH of an aqueous solution of $3.5\times {10}^{-3}M$ $\text{HBr}$

(c)

Interpretation Introduction

Interpretation:

The pH of the given aqueous solutions at ${\text{25}}^{\circ }\text{C}$ has to be calculated

Concept Information:

Strong acids:

In strong acids, the ionization of acid is complete. This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium.

pH definition:

The concentration of hydrogen ion is measured using $\text{pH}$ scale.  The acidity of aqueous solution is expressed by $\text{pH}$ scale.

The $\text{pH}$ of a solution is defined as the negative base-10 logarithm of the hydrogen or hydronium ion concentration.

$\text{pH}\text{=}{\text{-log[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$

On rearranging, the concentration of hydrogen ion ${\text{[H}}^{+}\text{]}$ can be calculated using pH as follows,

${\text{[H}}^{+}\text{]}\text{=}{\text{10}}^{\text{-pH}}$

To calculate: The pH of an aqueous solution of $9.3\times {10}^{-10}M$ $\text{HCl}$