   Chapter 16, Problem 88GQ

Chapter
Section
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%

Let’s calculate the degree of dissociation:

Percentionization10011100=0.11

Let’s calculate the concentration of acetic acid.

Ka= Cα2

Rearrange the formula is as follows.

C =Kα2

Ka of acetic acid is 1.85×10-5

α = 0.11

C =1.8×10-5(0.11)2=1

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