   # In glycine, the carboxylic acid group has K a = 4.3 × 10 −3 and the amino group has K b = 6.0 × 10 −5 . Use these equilibrium constant values to calculate the equilibrium constants for the following. a. H + 3 NCH 2 CO 2 − +H 2 O ⇌ H 2 NCH 2 CO 2 − +H 3 O + b. H 2 NCH 2 CO 2 − +H 2 O ⇌ H 2 NCH 2 CO 2 H+OH − c. H + 3 NCH 2 CO 2 H ⇌ 2 H + +H 2 NCH 2 CO 2 − ### 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 21, Problem 136AE
Textbook Problem
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## In glycine, the carboxylic acid group has Ka = 4.3 × 10−3 and the amino group has Kb = 6.0 × 10−5. Use these equilibrium constant values to calculate the equilibrium constants for the following.a. H + 3 NCH 2 CO 2 − +H 2 O ⇌ H 2 NCH 2 CO 2 − +H 3 O + b. H 2 NCH 2 CO 2 − +H 2 O ⇌ H 2 NCH 2 CO 2 H+OH − c. H + 3 NCH 2 CO 2 H ⇌ 2 H + +H 2 NCH 2 CO 2 −

(a)

Interpretation Introduction

Interpretation: The equilibrium constants for the following reactions are to be calculated.

Concept introduction: Equilibrium constant is defined as the ratio of the concentration of the products to the concentration of the reactants present at equilibrium in a reversible reaction at a given temperature. It is denoted by K and is a dimensionless quantity. Its value decide the direction of the chemical reaction, if the value of K is less than one the reaction will proceed towards left but when its value is greater than one the reaction will proceed in the right direction.

To determine: The equilibrium constant for the reaction.

### Explanation of Solution

Explanation

The equilibrium constant for the reaction is 1.6×10-10_ .

The given reaction is,

+H3NCH2CO2 + H2 H2NCH2CO2 + H3O+

In the given reaction, dissociation of an acid occurs.

The equilibrium constant expression for the above reaction is,

Ka=[H2NCH2CO2][H3O+][+H3NCH2COO]

Where,

• Ka is the acid dissociation constant

(b)

Interpretation Introduction

Interpretation: The equilibrium constants for the following reactions are to be calculated.

Concept introduction: Equilibrium constant is defined as the ratio of the concentration of the products to the concentration of the reactants present at equilibrium in a reversible reaction at a given temperature. It is denoted by K and is a dimensionless quantity. Its value decide the direction of the chemical reaction, if the value of K is less than one the reaction will proceed towards left but when its value is greater than one the reaction will proceed in the right direction.

To determine: The equilibrium constant for the reaction.

(c)

Interpretation Introduction

Interpretation: The equilibrium constants for the following reactions are to be calculated.

Concept introduction: Equilibrium constant is defined as the ratio of the concentration of the products to the concentration of the reactants present at equilibrium in a reversible reaction at a given temperature. It is denoted by K and is a dimensionless quantity. Its value decide the direction of the chemical reaction, if the value of K is less than one the reaction will proceed towards left but when its value is greater than one the reaction will proceed in the right direction.

To determine: The equilibrium constant for the reaction.

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