Chapter 4, Problem 109GQ

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# (a) What is the pH of a 0.105 M HCl solution? (b) What is the hydronium ion concentration in a solution with a pH of 2.56? Is the solution acidic or basic? (c) A solution has a pH of 9.67. What is the hydronium ion concentration in the solution? Is the solution acidic or basic? (d) A 10.0-mL sample of 2.56 M HCl is diluted with water to 250. mL What is the pH of the dilute solution?

(a)

Interpretation Introduction

Interpretation:

pH of 0.105 M HCl solution has to be determined.

Concept introduction:

• Strong acids dissociates completely into ions in solution but weak acids do not.
• 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.
• Amountofsubstance=Concnetrationofthesubstance×Volume
Explanation

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

â€‚Â pHâ€‰â€‰=â€‰â€‰-log10â€‰[H3O+]

It possible to substitute the value of H+ instead of H3O+

HCl is a strong acid. Â So the concentration of H+â€‰â€‰andâ€‰â€‰HCl will be equal

(b)

Interpretation Introduction

Interpretation:

Hydronium ion concentration in a solution with a pHof2.56 has to be determined and the solution is whether acidic or basic has to be ascertained.

Concept introduction:

• Strong acids dissociates completely into ions in solution but weak acids do not.
• 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 hydronium ion concentration in a solution with a pHof9.67 has to be determined and the solution is whether acidic or basic has to be ascertained.

Concept introduction:

• Strong acids dissociates completely into ions in solution but weak acids do not.
• 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 pH of the dilute solution has to be determined.

Concept introduction:

• Strong acids dissociates completely into ions in solution but weak acids do not.
• 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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