   Chapter 16, Problem 16.83QP General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343

Solutions

Chapter
Section General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343
Textbook Problem

How many moles of sodium acetate must be added to 2.0 L of 0.10 M acetic acid to give a solution that has a pH equal to 4.90? Ignore the volume change due to the addition of sodium acetate.

Interpretation Introduction

Interpretation:

The moles of sodium acetate which is needed to be added to 2.0 L of 0.10 M acetic acid to give a solution that has a pH equal to 4.90 has to be calculated

Concept Introduction:

The pH can be calculated using Henderson-Hasselbalch equation as follows,

pH = pKa + log[conjugate base][weak acid]pH = pKa + log[A-][HA]

To Calculate: The moles of sodium acetate which is needed to be added to 2.0 L of 0.10 M acetic acid to give a solution that has a pH equal to 4.90

Explanation

Given data:

The concentration of acetic acid = 0.10 M

The volume of acetic acid = 2.0 L

The pH of the solution is 4.90

Mole calculation:

Let us represent, acetic acid as HOAc and sodium acetate as Na+OAc-

We know that,

pKa = -log Ka

The Ka for acetic acid is 1.7×105

The moles of sodium acetate that is needed can be calculated using the Henderson-Hasselbalch equation as follows,

pH = pKa + log[conjugate base][weak acid]    4.90 = -log(1.7×105) + log[OAc-]0

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