Chapter 4, Problem 59PS

(a)

Interpretation Introduction

Interpretation:

The $pH$ of $1.00$ has to be converted into $\left[H_3{O}^{+}\right]$ and whether it is acidic or basic has to be determined.

Concept introduction:

• $\text{pH}$ of a solution is the negative of the base $\text{-10}$ logarithm of the hydronium ion concentration.

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

• Concentration of hydronium ion $\left[{\text{H}}_{\text{3}}{\text{O}}^{\text{+}}\right]\text{=}{\text{10}}^{\text{-pH}}$
• For an acidic solution $\text{pH}\text{<7}$ and for a basic solution $\text{pH>}\text{7}$.

(b)

Interpretation Introduction

Interpretation:

The $pH$ of $10.50$ has to be converted into $\left[H_3{O}^{+}\right]$ and whether it is acidic or basic has to be determined.

Concept introduction:

• $\text{pH}$ of a solution is the negative of the base $\text{-10}$ logarithm of the hydronium ion concentration.

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

• Concentration of hydronium ion $\left[{\text{H}}_{\text{3}}{\text{O}}^{\text{+}}\right]\text{=}{\text{10}}^{\text{-pH}}$
• For an acidic solution $\text{pH}\text{<7}$ and for a basic solution $\text{pH>}\text{7}$.

(c)

Interpretation Introduction

Interpretation:

The $\left[H_3{O}^{+}\right]$ has to be converted into $pH$ and whether it is acidic or basic has to be determined.

Concept introduction:

• $\text{pH}$ of a solution is the negative of the base $\text{-10}$ logarithm of the hydronium ion concentration.

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

• Concentration of hydronium ion $\left[{\text{H}}_{\text{3}}{\text{O}}^{\text{+}}\right]\text{=}{\text{10}}^{\text{-pH}}$
• For an acidic solution $\text{pH}\text{<7}$ and for a basic solution $\text{pH>}\text{7}$.

(d)

Interpretation Introduction

Interpretation:

The $\left[H_3{O}^{+}\right]$ has to be converted into $pH$ and whether it is acidic or basic has to be determined.

Concept introduction:

• $\text{pH}$ of a solution is the negative of the base $\text{-10}$ logarithm of the hydronium ion concentration.

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

• Concentration of hydronium ion $\left[{\text{H}}_{\text{3}}{\text{O}}^{\text{+}}\right]\text{=}{\text{10}}^{\text{-pH}}$
• For an acidic solution $\text{pH}\text{<7}$ and for a basic solution $\text{pH>}\text{7}$.