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ChemistryChemistry: An Atoms First Approach2nd Edition
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Calculate the value for the equilibrium constant for each of the following aqueous reactions. a. NH 3 +H 3 O + ⇌ NH 4 + +H 2 O b. NO 2 − + H 3 O + ⇌ HNO 2 + H 2 O c. NH 4 + + OH − ⇌ NH 3 + H 2 O d. HNO 2 + OH − ⇌ H 2 O+NO 2 −

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 13, Problem 160AE
Textbook Problem
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Calculate the value for the equilibrium constant for each of the following aqueous reactions.

a. NH 3 +H 3 O + ⇌ NH 4 + +H 2 O

b. NO 2 − + H 3 O + ⇌ HNO 2 + H 2 O

c. NH 4 + + OH − ⇌ NH 3 + H 2 O

d. HNO 2 + OH − ⇌ H 2 O+NO 2 −

(a)

Interpretation Introduction

Interpretation:

The equilibrium constant is to be calculated for NH3+H3O+⇌NH4++H2O.

Concept introduction:

The Kb equilibrium constant is the ratio of product of equilibrium concentrations of product to the equilibrium concentration of reactant base.

Explanation of Solution

The given reaction is,

    NH3+H3O+⇌NH4++H2O

Formula

The expression for the equilibrium constant for the given reaction is,

  K=[NH4+][NH3][H3O+]

Multiply [OH−] in the numerator and denominator of right hand side,

  K=[NH4+][NH3][H3O+]×[OH−][OH−]=[NH4+][OH−][

(b)

Interpretation Introduction

Interpretation:

The equilibrium constant is to be calculated for NO2−+H3O+⇌HNO2+H2O.

Concept introduction:

The Kb equilibrium constant is the ratio of product of equilibrium concentrations of product to the equilibrium concentration of reactant base.

(c)

Interpretation Introduction

Interpretation:

The equilibrium constant is to be calculated for NH4++OH−⇌NH3+H2O.

Concept introduction:

The Kb equilibrium constant is the ratio of product of equilibrium concentrations of product to the equilibrium concentration of reactant base.

(d)

Interpretation Introduction

Interpretation:

The equilibrium constant is to be calculated for HNO2+OH−⇌H2O+NO2−.

Concept introduction:

The Kb equilibrium constant is the ratio of product of equilibrium concentrations of product to the equilibrium concentration of reactant base.

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Ch. 13 - Define each of the following: a. Arrhenius acid b....Ch. 13 - Define or illustrate the meaning of the following...Ch. 13 - Define or illustrate the meaning of the following...Ch. 13 - How is acid strength related to the value of Ka?...Ch. 13 - Two strategies are followed when solving for the...Ch. 13 - Two strategies are also followed when solving for...Ch. 13 - Table 13-4 lists the stepwise Ka values for some...Ch. 13 - For conjugate acidbase pairs, how are Ka and Kb...Ch. 13 - What is a salt? List some anions that behave as...Ch. 13 - For oxyacids, how does acid strength depend on a....
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