   # Calculate [OH − ], [H + ], and the pH of 0.40 M solutions of each of the following amines (the K b values are found in Table 13-3). a. aniline b. methylamine ### 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 98E
Textbook Problem
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## Calculate [OH−], [H+], and the pH of 0.40 M solutions of each of the following amines (the Kb values are found in Table 13-3).a. anilineb. methylamine

(a)

Interpretation Introduction

Interpretation: The pH,[H+] and [OH] of the given amines is to be calculated.

Concept introduction: The pH of a solution is defined as a figure that expresses the acidity of the alkalinity of a given solution.

The pOH of a solution is calculated by the formula, pOH=log[OH]

The sum, pH+pOH=14

At equilibrium, the equilibrium constant expression is expressed by the formula,

Kb=ConcentrationofproductsConcentrationofreactants

To determine: The pH,[H+] and [OH] of C6H5NH2 .

### Explanation of Solution

Explanation

The equilibrium constant expression for the given reaction is,

Kb=[C6H5NH3+][OH][C6H5NH2]

The reaction involved is,

C6H5NH2(aq)+H2O(l)C6H5NH3+(aq)+OH(aq)

At equilibrium, the equilibrium constant expression is expressed by the formula,

Kb=ConcentrationofproductsConcentrationofreactants

Where,

• Kb is the base ionization constant.

The equilibrium constant expression for the given reaction is,

Kb=[C6H5NH3+][OH][C6H5NH2] (1)

The [OH] is 1.23×10-5M_ .

The change in concentration of C6H5NH2 is assumed to be x .

The liquid components do not affect the value of the rate constant.

The ICE table for the stated reaction is,

C6H5NH2(aq)C6H5NH3+(aq)+OH(aq)Inititialconcentration0.4000Changex+x+xEquilibriumconcentration0.40xxx

The equilibrium concentration of [C6H5NH2] is (0.40x)M .

The equilibrium concentration of [C6H5NH3+] is xM .

The equilibrium concentration of [OH] is xM .

The Kb value is given to be 3.8×1010 .

Substitute the value of Kb , [C6H5NH2] , [C6H5NH3+] and [OH] in equation (1)

(b)

Interpretation Introduction

Interpretation: The pH,[H+] and [OH] of the given amines is to be calculated.

Concept introduction: The pH of a solution is defined as a figure that expresses the acidity of the alkalinity of a given solution.

The pOH of a solution is calculated by the formula, pOH=log[OH]

The sum, pH+pOH=14

At equilibrium, the equilibrium constant expression is expressed by the formula,

Kb=ConcentrationofproductsConcentrationofreactants

To determine: The pH,[H+] and [OH] of CH3NH2 .

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