   # Calculate [OH − ] , [H + ], and the pH of 0.20 M solutions of each of the following amines. a. triethylamine [(C 2 H 5 ) 3 N, K b = 4.0 × 10 −4 ] b. hydroxylamine (HONH 2 , K b = 1.1 × 10 −8 ) ### 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 97E
Textbook Problem
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## Calculate [OH−], [H+], and the pH of 0.20 M solutions of each of the following amines.a. triethylamine [(C2H5)3N, Kb = 4.0 × 10−4]b. hydroxylamine (HONH2, Kb = 1.1 × 10−8)

(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 (C2H5)3N .

### Explanation of Solution

Explanation

The equilibrium constant expression for the given reaction is,

Kb=[(C2H5)3NH+][OH][(C2H5)3N]

The reaction involved is,

(C2H5)3N(aq)+H2O(l)(C2H5)3NH+(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=[(C2H5)3NH+][OH][(C2H5)3N] (1)

The [OH] is 8.94×10-3M_ .

The change in concentration of (C2H5)3N 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,

(C2H5)3N(aq)(C2H5)3NH+(aq)+OH(aq)Inititialconcentration0.2000Changex+x+xEquilibriumconcentration0.20xxx

The equilibrium concentration of [(C2H5)3N] is (0.20x)M .

The equilibrium concentration of [(C2H5)3NH+] is xM .

The equilibrium concentration of [OH] is xM .

The Kb value is given to be 4.0×104 .

Substitute the value of Kb , [(C2H5)3N] , [(C2H5)3NH+] 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 HONH2 .

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