Chapter 9, Problem 68P

Interpretation Introduction

(a)

Interpretation:

The pH of solution with $\text{1}{\text{.0 × 10}}^{\text{-2}}\text{ M}$ of ${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}{}_{\text{(aq)}}\text{]}$ ions needs to be determined.

Concept Introduction:

A substance is said to be acidic if it can give hydrogen ions ( ${\text{H}}^{\text{+}}$ ) whereas a base is said to be a substance that can give ${\text{OH}}^{\text{-}}$ ion. This theory of acid and base is called the Arrhenius theory of acid and base.

Another theory that is purposed by Bronsted and Lowery is called Bronsted-Lowry acid-base theory. It states that acid can give ${\text{H}}^{\text{+}}$ ions whereas a base can accept the ${\text{H}}^{\text{+}}$ ion in its solution. Hence this theory is entirely based on the presence of ${\text{H}}^{\text{+}}$ ion in the given substance.

The acidic and basic nature of the solution can be expressed in terms of pH of the solution. The range of pH lies from 0 to 14. The pH value from 0 to 7 indicates an acidic solution whereas the pH value from 7 to 14 stands for a basic solution. A neutral solution can be expressed as pH 7. It can be calculated with the help of concentration ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ ions and can be formulated as:

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

Interpretation Introduction

(b)

Interpretation:

The pH of solution with $\text{2}{\text{.0 × 10}}^{\text{-5}}\text{ M}$ of ${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}{}_{\text{(aq)}}\text{]}$ ions needs to be determined.

Concept Introduction:

A substance is said to be acidic if it can give hydrogen ions ( ${\text{H}}^{\text{+}}$ ) whereas a base is said to be a substance that can give ${\text{OH}}^{\text{-}}$ ion. This theory of acid and base is called the Arrhenius theory of acid and base.

Another theory that is purposed by Bronsted and Lowery is called Bronsted-Lowry acid-base theory. It states that acid can give ${\text{H}}^{\text{+}}$ ions whereas a base can accept the ${\text{H}}^{\text{+}}$ ion in its solution. Hence this theory is entirely based on the presence of ${\text{H}}^{\text{+}}$ ion in the given substance.

The acidic and basic nature of the solution can be expressed in terms of pH of the solution. The range of pH lies from 0 to 14. The pH value from 0 to 7 indicates an acidic solution whereas the pH value from 7 to 14 stands for a basic solution. A neutral solution can be expressed as pH 7. It can be calculated with the help of concentration ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ ions and can be formulated as:

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

Interpretation Introduction

(c)

Interpretation:

The pH of solution with $\text{ 1}{\text{.7 × 10}}^{\text{-11}}\text{ M}$ of ${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}{}_{\text{(aq)}}\text{]}$ ions needs to be determined.

Concept Introduction:

A substance is said to be acidic if it can give hydrogen ions ( ${\text{H}}^{\text{+}}$ ) whereas a base is said to be a substance that can give ${\text{OH}}^{\text{-}}$ ion. This theory of acid and base is called the Arrhenius theory of acid and base.

Another theory that is purposed by Bronsted and Lowery is called Bronsted-Lowry acid-base theory. It states that acid can give ${\text{H}}^{\text{+}}$ ions whereas a base can accept the ${\text{H}}^{\text{+}}$ ion in its solution. Hence this theory is entirely based on the presence of ${\text{H}}^{\text{+}}$ ion in the given substance.

The acidic and basic nature of the solution can be expressed in terms of pH of the solution. The range of pH lies from 0 to 14. The pH value from 0 to 7 indicates an acidic solution whereas the pH value from 7 to 14 stands for a basic solution. A neutral solution can be expressed as pH 7. It can be calculated with the help of concentration ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ ions and can be formulated as:

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

Interpretation Introduction

(d)

Interpretation:

The pH of solution with $\text{1}{\text{.1 × 10}}^{\text{-4}}\text{ M}$ of ${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}{}_{\text{(aq)}}\text{]}$ ions needs to be determined.

Concept Introduction:

A substance is said to be acidic if it can give hydrogen ions ( ${\text{H}}^{\text{+}}$ ) whereas a base is said to be a substance that can give ${\text{OH}}^{\text{-}}$ ion. This theory of acid and base is called the Arrhenius theory of acid and base.

Another theory that is purposed by Bronsted and Lowery is called Bronsted-Lowry acid-base theory. It states that acid can give ${\text{H}}^{\text{+}}$ ions whereas a base can accept the ${\text{H}}^{\text{+}}$ ion in its solution. Hence this theory is entirely based on the presence of ${\text{H}}^{\text{+}}$ ion in the given substance.

The acidic and basic nature of the solution can be expressed in terms of pH of the solution. The range of pH lies from 0 to 14. The pH value from 0 to 7 indicates an acidic solution whereas the pH value from 7 to 14 stands for a basic solution. A neutral solution can be expressed as pH 7. It can be calculated with the help of concentration ${\text{H}}_{\text{3}}{\text{O}}^{\text{+}}$ ions and can be formulated as:

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