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Chemistry & Chemical Reactivity

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

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

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

  1. (a) What is the pH of a 0.105 M HCl solution?
  2. (b) What is the hydronium ion concentration in a solution with a pH of 2.56? Is the solution acidic or basic?
  3. (c) A solution has a pH of 9.67. What is the hydronium ion concentration in the solution? Is the solution acidic or basic?
  4. (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.

  pH=-log10[H3O+]

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

HCl is a strong acid.  So the concentration of H+andHCl 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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