Chapter 16, Problem 88GQ

### 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

# In a particular solution, acetic acid is 11% ionized at 25 °C. Calculate the pH of the solution and the mass of acetic acid dissolved to yield 1.00L of solution.

Interpretation Introduction

Interpretation:

The pH and mass of acetic acid has to be determined when it is dissolved to yield 1.00L of solution at 250C, acetic acid is 11% ionized.

Concept introduction:

The relatioship between acid dissociation constant and degree of dissociation is as follows.

Ka= Cα2Ka= Acid dissociation constantC  = Concentration of acidα   = Degree of dissociation

Explanation

The given percent of ionization = 11%

Letâ€™s calculate the degree of dissociation:

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 Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â  =Â Percentionization100=Â 11100=0.11

Letâ€™s calculate the concentration of acetic acid.

Ka=Â CÎ±2

Rearrange the formula is as follows.

CÂ =KÎ±2

Ka of acetic acid is 1.85Ã—10-5

Î±Â =Â 0.11

CÂ =1.8Ã—10-5(0.11)2=1

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