   # Calculate the molar concentration of H 3 O + in water solutions with the following OH − molar concentrations: a. 6.9 × 10 − 5 b. 0.074 c. 4.9 d. 1.7 × 10 − 3 e. 9.2 × 10 − 9 ### Chemistry for Today: General, Orga...

9th Edition
Spencer L. Seager + 2 others
Publisher: Cengage Learning
ISBN: 9781305960060

#### Solutions

Chapter
Section ### Chemistry for Today: General, Orga...

9th Edition
Spencer L. Seager + 2 others
Publisher: Cengage Learning
ISBN: 9781305960060
Chapter 9, Problem 9.30E
Textbook Problem
1 views

## Calculate the molar concentration of H 3 O + in water solutions with the following OH − molar concentrations:a. 6.9 × 10 − 5 b. 0.074 c. 4.9 d. 1.7 × 10 − 3 e. 9.2 × 10 − 9

Interpretation Introduction

(a)

Interpretation:

The molar concentration of H3O+ in water solutions with the given OH molar concentrations is to be calculated.

Concept introduction:

The water undergoes self-ionization which can be represented by the reaction,

H2O(l)+H2O(l)H3O+(aq)+OH(aq)

The ionization constant of water is represented as,

K=[H3O+][OH][H2O][H2O]

The concentration of water remains constant and the self-ionization constant of water becomes,

Kw=[H3O+][OH]Kw=(1.0×107mol/L)(1.0×107mol/L)Kw=1.0×1014(mol/L)2

### Explanation of Solution

The ionic product of water Kw is,

Kw=[H3O+][OH]

The value of Kw is 1.0×1014(mol/L)2.

The given OH molar concentration is 6.9×105mol/L. Substitute this value in the formula for ionic product.

1.0×1014(mol/L)2=[H3O+]6

Interpretation Introduction

(b)

Interpretation:

The molar concentration of H3O+ in water solutions with the given OH molar concentrations is to be calculated.

Concept introduction:

The water undergoes self-ionization which can be represented by the reaction,

H2O(l)+H2O(l)H3O+(aq)+OH(aq)

The ionization constant of water is represented as,

K=[H3O+][OH][H2O][H2O]

The concentration of water remains constant and the self-ionization constant of water becomes,

Kw=[H3O+][OH]Kw=(1.0×107mol/L)(1.0×107mol/L)Kw=1.0×1014(mol/L)2

Interpretation Introduction

(c)

Interpretation:

The molar concentration of H3O+ in water solutions with the given OH molar concentrations is to be calculated.

Concept introduction:

The water undergoes self-ionization which can be represented by the reaction,

H2O(l)+H2O(l)H3O+(aq)+OH(aq)

The ionization constant of water is represented as,

K=[H3O+][OH][H2O][H2O]

The concentration of water remains constant and the self-ionization constant of water becomes,

Kw=[H3O+][OH]Kw=(1.0×107mol/L)(1.0×107mol/L)Kw=1.0×1014(mol/L)2

Interpretation Introduction

(d)

Interpretation:

The molar concentration of H3O+ in water solutions with the given OH molar concentrations is to be calculated.

Concept introduction:

The water undergoes self-ionization which can be represented by the reaction,

H2O(l)+H2O(l)H3O+(aq)+OH(aq)

The ionization constant of water is represented as,

K=[H3O+][OH][H2O][H2O]

The concentration of water remains constant and the self-ionization constant of water becomes,

Kw=[H3O+][OH]Kw=(1.0×107mol/L)(1.0×107mol/L)Kw=1.0×1014(mol/L)2

Interpretation Introduction

(e)

Interpretation:

The molar concentration of H3O+ in water solutions with the given OH molar concentrations is to be calculated.

Concept introduction:

The water undergoes self-ionization which can be represented by the reaction,

H2O(l)+H2O(l)H3O+(aq)+OH(aq)

The ionization constant of water is represented as,

K=[H3O+][OH][H2O][H2O]

The concentration of water remains constant and the self-ionization constant of water becomes,

Kw=[H3O+][OH]Kw=(1.0×107mol/L)(1.0×107mol/L)Kw=1.0×1014(mol/L)2

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