   # a. The principal equilibrium in a solution of NaHCO 3 is HCO 3 − ( a q ) + HCO 3 − ( a q ) ⇌ H 2 CO 3 ( a q ) + CO 3 2 − ( a q ) Calculate the value of the equilibrium constant for this reaction. b. At equilibrium, what is the relationship between [H 2 CO 3 ] and [CO 3 2− ]? c. Using the equilibrium H 2 CO 3 ( a q ) ⇌ 2 H + ( a q ) + CO 3 2 − ( a q ) derive an expression for the pH of the solution in terms of K a 1 and K a 2 using the result from part b. d. What is the pH of a solution of NaHCO 3 ? ### Chemistry: An Atoms First Approach

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

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 13, Problem 184CP
Textbook Problem
1 views

## a. The principal equilibrium in a solution of NaHCO3 is HCO 3 − ( a q ) + HCO 3 − ( a q ) ⇌ H 2 CO 3 ( a q ) + CO 3 2 − ( a q ) Calculate the value of the equilibrium constant for this reaction.b. At equilibrium, what is the relationship between [H2CO3] and [CO32−]?c. Using the equilibrium H 2 CO 3 ( a q ) ⇌ 2 H + ( a q ) + CO 3 2 − ( a q ) derive an expression for the pH of the solution in terms of K a 1 and K a 2 using the result from part b.d. What is the pH of a solution of NaHCO3?

(a)

Interpretation Introduction

Interpretation: The value of equilibrium constant, relationship between [H2CO3] and [CO32] at equilibrium,. expression for pH in terms of Ka1 and Ka2, pH of NaHCO3.

Concept introduction: The equilibrium constant is defined as the numeric number that describes the relationship between amount of product and amount of reactant at equilibrium. The pH is the scale that measures the power of hydrogen ion concentration of a species.

To determine: The value of equilibrium constant.

### Explanation of Solution

Explanation

The given reaction is,

HCO3+HCO3H2CO3+CO32

The equilibrium constant expression is,

Keq=[concentrationofproduct][concentrationofreactants]

The equilibrium constant expression for the given reaction is,

Keq=[H2CO3][CO32][HCO3][HCO3]

Multiply numerator and denominator by [H+].

Keq=[H2CO3][CO32][HCO3][HCO3][H+][H+] (1)

Rearrange the above equation (1)

Keq=[H+][CO32][H2CO3][HCO3][H+

(b)

Interpretation Introduction

Interpretation: The value of equilibrium constant, relationship between [H2CO3] and [CO32] at equilibrium,. expression for pH in terms of Ka1 and Ka2, pH of NaHCO3.

Concept introduction: The equilibrium constant is defined as the numeric number that describes the relationship between amount of product and amount of reactant at equilibrium. The pH is the scale that measures the power of hydrogen ion concentration of a species.

To determine: The relationship between [H2CO3] and [CO32] at equilibrium.

(c)

Interpretation Introduction

Interpretation: The value of equilibrium constant, relationship between [H2CO3] and [CO32] at equilibrium,. expression for pH in terms of Ka1 and Ka2, pH of NaHCO3.

Concept introduction: The equilibrium constant is defined as the numeric number that describes the relationship between amount of product and amount of reactant at equilibrium. The pH is the scale that measures the power of hydrogen ion concentration of a species.

To determine: The expression for pH in terms of Ka1 and Ka2.

(d)

Interpretation Introduction

Interpretation: The value of equilibrium constant, relationship between [H2CO3] and [CO32] at equilibrium,. expression for pH in terms of Ka1 and Ka2, pH of NaHCO3.

Concept introduction: The equilibrium constant is defined as the numeric number that describes the relationship between amount of product and amount of reactant at equilibrium. The pH is the scale that measures the power of hydrogen ion concentration of a species.

To determine: The pH of NaHCO3.

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