   Chapter 9, Problem 9.27E Chemistry for Today: General, Orga...

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

Solutions

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

9th Edition
Spencer L. Seager + 2 others
ISBN: 9781305960060
Textbook Problem

Calculate the molar concentration of OH − in water solutions with the following H 3 O + molar concentrations:a. 1.0 × 10 − 6 b. 4.8 × 10 − 4 c. 6.2 × 10 − 10 d. 1.4 e. 0.038

Interpretation Introduction

(a)

Interpretation:

The molar concentration of OH in water solutions with the given H3O+ 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

The ionic product of water Kw is,

Kw=[H3O+][OH]

The value of Kw is 1.0×1014(mol/L)2.

The given H3O+ molar concentration is 1.0×106mol/L. Substitute this value in the formula for ionic product.

1.0×1014(mol/L)2=1

Interpretation Introduction

(b)

Interpretation:

The molar concentration of OH in water solutions with the given H3O+ 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 OH in water solutions with the given H3O+ 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 OH in water solutions with the given H3O+ 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 OH in water solutions with the given H3O+ 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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