   Chapter 4, Problem 60PS

Chapter
Section
Textbook Problem

Make the following conversions. In each case, tell whether the solution is acidic or basic. (a)

Interpretation Introduction

Interpretation:

The [H3O+] has to be converted into pH and whether it is acidic or basic has to be determined.

Concept introduction:

• pH of a solution is the negative of the base -10 logarithm of the hydronium ion concentration.

pH=-log[H3O+]

• Concentration of hydronium ion [H3O+]=10-pH
• For an acidic solution pH<7 and for a basic solution pH>7.
Explanation

Acidic and basic nature of any substance can be predicted from their pH value.

pH of the solution a can be determined  by using the equation,

pH = - log[H3O+]pH

(b)

Interpretation Introduction

Interpretation:

The [H3O+] has to be converted into pH and whether it is acidic or basic has to be determined.

Concept introduction:

• pH of a solution is the negative of the base -10 logarithm of the hydronium ion concentration.

pH=-log[H3O+]

• Concentration of hydronium ion [H3O+]=10-pH
• For an acidic solution pH<7 and for a basic solution pH>7.

(c)

Interpretation Introduction

Interpretation:

The pH of 5.25 has to be converted into [H3O+] and whether it is acidic or basic has to be determined.

Concept introduction:

• pH of a solution is the negative of the base -10 logarithm of the hydronium ion concentration.

pH=-log[H3O+]

• Concentration of hydronium ion [H3O+]=10-pH
• For an acidic solution pH<7 and for a basic solution pH>7.

(d)

Interpretation Introduction

Interpretation:

The [H3O+] has to be converted into pH and whether it is acidic or basic has to be determined.

Concept introduction:

• pH of a solution is the negative of the base -10 logarithm of the hydronium ion concentration.

pH=-log[H3O+]

• Concentration of hydronium ion [H3O+]=10-pH
• For an acidic solution pH<7 and for a basic solution pH>7.

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