   # Calculate the pH of each of the following solutions. a. 0.100 M HONH 2 ( K b = 1.1 × 10 −8 ) b. 0.100 M HONH 3 Cl c. pure H 2 O d. a mixture containing 0.100 M HONH 2 and 0.100 M HONH 3 Cl ### 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 14, Problem 22E
Textbook Problem
61 views

## Calculate the pH of each of the following solutions.a. 0.100 M HONH2 (Kb= 1.1 × 10−8)b. 0.100 M HONH3Clc. pure H2Od. a mixture containing 0.100 M HONH2 and 0.100 M HONH3Cl

(a)

Interpretation Introduction

Interpretation:

The pH of the given solutions is to be calculated.

Concept introduction:

The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution.

The pH of a solution is calculated by the formula, pH=log[H+]

The sum, pH+pOH=14

The value of Kw is calculated by the formula,

Kw=KaKb

### Explanation of Solution

Explanation

To determine the [OH] of the given solution.

The dominant equilibrium reaction that takes place in the given case is,

HONH2(aq)+H2O(l)HONH3+(aq)+OH(aq)

The change in the concentration of HONH2 is assumed to be x .

The ICE table is formed for the given reaction.

HONH2(aq)HONH3+(aq)+OH(aq)Initialconcentration0.10000Changex+x+xEquilibriumconcentration0.100xxx

The equilibrium concentration of [HONH2(aq)] is (0.100x)M .

The equilibrium concentration of [HONH3+(aq)] is xM .

The equilibrium concentration of [OH] is xM .

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=[HONH3+][OH][HONH2]

The value of Kb is given to be 1

(b)

Interpretation Introduction

Interpretation:

The pH of the given solutions is to be calculated.

Concept introduction:

The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution.

The pH of a solution is calculated by the formula, pH=log[H+]

The sum, pH+pOH=14

The value of Kw is calculated by the formula,

Kw=KaKb

(c)

Interpretation Introduction

Interpretation:

The pH of the given solutions is to be calculated.

Concept introduction:

The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution.

The pH of a solution is calculated by the formula, pH=log[H+]

The sum, pH+pOH=14

The value of Kw is calculated by the formula,

Kw=KaKb

(d)

Interpretation Introduction

Interpretation:

The pH of the given solutions is to be calculated.

Concept introduction:

The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution.

The pH of a solution is calculated by the formula, pH=log[H+]

The sum, pH+pOH=14

The value of Kw is calculated by the formula,

Kw=KaKb

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