Chapter 16, Problem 107GQ

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# To what volume should 1.00 × 102 mL of any weak acid, HA, with a concentration 0.20 M be diluted to double the percentage ionization?

Interpretation Introduction

Interpretation:

The volume has to be determined when diluted to double the percentage of ionization.

Concept introduction:

Equilibrium constants:

The equilibrium constant is used to quantitative measurement of the strength of the acid and bases in the water.

Ka is an acid constant for equilibrium reactions.

HA + H2OH3O++ A-Ka[H3O+][A-][HA]

Kb is base constant for equilibrium reaction.

BOH + H2OB++ OH-Ka[B+][OH-][BOH]

Explanation

The equlibrium chemical reaction is as follows.

HAâ‡ŒH++A-

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â HAÂ Â â‡ŒH++A-Equilibrium(M)Â Â Â C(1-Î±)Â Â Â Â Â Â Â Â Î±Â Â Â Â Â Î±

Hence,

Ka=Â [H+][A-][HA]=Â Î±CÃ—Î±CC(1-Î±)=Â Î±2C1-Î±

Ka=Â Î±2C1-Â Î± (1)

From the given,

VÂ =1.0Ã—102Â mLConcentrationÂ =Â 0.20Â M

Substitute the values in the equation (1)

C=Â 0.20Â mol1.0Ã—1021000LÂ =Â 2Â M

From equation (1)

Ka=Â Î±2C1-Â Î±Ka=Â Î±2(2)1-Â Î±â€‰â€‰

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