Quantitative Chemical Analysis
Quantitative Chemical Analysis
9th Edition
ISBN: 9781464135385
Author: Daniel C. Harris
Publisher: W. H. Freeman
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Chapter 9, Problem 9.41P

a)

Interpretation Introduction

Interpretation:

The chemical reaction with equilibrium constants Kb and Ka for Imidazole and Imidazole hydrochloride have to be written.

Concept Introduction:

Acid dissociation constant:

Consider a weak-acid equilibrium reaction,

HAKaH++A-

The acid dissociation constant Ka can be given as,

Ka=[H+][A-][HA]

A weak acid is one that doesn’t undergo completion.

Base dissociation constant:

Consider a reaction of weak base,

B+H2OKbBH++OH-

The value of Kb can be calculated as,

Kb=[BH+][OH-][B]

Where Kb is called as base dissociation constant.

To write the chemical reaction with equilibrium constants Kb and Ka for Imidazole and Imidazole hydrochloride

a)

Expert Solution
Check Mark

Explanation of Solution

The chemical reaction with equilibrium constants Kb and Ka for Imidazole and Imidazole hydrochloride can be written as,

Quantitative Chemical Analysis, Chapter 9, Problem 9.41P

b)

Interpretation Introduction

Interpretation:

The pH of a solution has to be calculated.

Concept Introduction:

Henderson-Hasselbalch equation:

Henderson- Hasselbalch equation is rearranged form of acid dissociation expression.

For acid:

Consider an acidic reaction:

HAKaH++A-

The Henderson- Hasselbalch equation for an acidic reaction can be given as,

pH=pKa+log[A-][HA]

b)

Expert Solution
Check Mark

Answer to Problem 9.41P

The pH of a solution is 7.18 .

Explanation of Solution

Given,

Mass of Imidazole = 1.00g

Mass of Imidazole hydrochloride = 1.00g

Volume to be diluted = 1.00ml

Formula mass of Imidazole = 68.08g

Formula mass of Imidazole hydrochloride = 104.54

pKa=6.993

The pH can be calculated as,

pH=pKa+log[A-][HA]pH=6.993+log1.00/68.081.00/104.54pH=7.18

The pH of a solution = 7.18

c)

Interpretation Introduction

Interpretation:

The pH of a solution has to be calculated.

Concept Introduction:

Henderson-Hasselbalch equation:

Henderson- Hasselbalch equation is rearranged form of acid dissociation expression.

For acid:

Consider an acidic reaction:

HAKaH++A-

The Henderson- Hasselbalch equation for an acidic reaction can be given as,

pH=pKa+log[A-][HA]

c)

Expert Solution
Check Mark

Answer to Problem 9.41P

The pH of a solution is 7.00 .

Explanation of Solution

Given,

Mass of Imidazole = 1.00g

Mass of Imidazole hydrochloride = 1.00g

Volume to be diluted = 1.00ml

Volume and Molarity of HClO4 = 2.30mland1.07M

Formula mass of Imidazole = 68.08g

Formula mass of Imidazole hydrochloride = 104.54

The pH can be calculated as,

B+H+BH+_Initialmoles14.692.469.57Finalmoles12.23-12.03

pH=pKa+log[A-][HA]pH=6.993+log12.2312.03pH=7.00

The pH of a solution = 7.00

d)

Interpretation Introduction

Interpretation:

The volume in millimetres that is required to be add has to be given.

To give the required volume to be added in millimetres.

d)

Expert Solution
Check Mark

Answer to Problem 9.41P

The required volume that is to be added is 6.86ml .

Explanation of Solution

In order to obtain pH=pKa , the Imidazole should be half neutralized.

Because there are 14.69mmol of Imidazole, the volume that is required of 1.07MHClO4 to be added to Imidazole is calculated as,

Volume of HClO4 = 12(14.69)=7.34mmol=6.86ml

The volume that is required of 1.07MHClO4 to be added to Imidazole = 6.86ml

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