Part 1In every part of the experiment, the [H3O+] is obtained from the pH, and C₂H₂O₂ is abbreviated AcIn Part 1, [Ac¯] = [H3O+], and [HAc] = (Label Concentration - [H3O+])[Ac] 1.15 x 10^-3b) 1.0 M HAC:pHKa=2.94[H3O+][H₂O+] [AC][HAC]1.15 x 10^-31.32 x 10^-6[HAC] 0.999 Repeat the calculation for the value of the K in Part 1b, only this time, do not subtract the [H3O+] from the label con-acentration of HAc. How does the value compare to the one you had originally?

Concept based on the acid dissociation constant of weak acids and finding out the acid dissociation…

Answered: Repeat the calculation for the value of…

Repeat the calculation for the value of the K in Part 1b, only this time, do not subtract the [H3O+] from the label con- centration of HAc. How does the value compare to the one you had originally?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Part 1
In every part of the experiment, the [H3O+] is obtained from the pH, and C₂H₂O₂ is abbreviated Ac
In Part 1, [Ac¯] = [H3O+], and [HAc] = (Label Concentration - [H3O+])
[Ac] 1.15 x 10^-3
b) 1.0 M HAC:
pH
Ka
=
2.94
[H3O+]
[H₂O+] [AC]
[HAC]
1.15 x 10^-3
1.32 x 10^-6
[HAC] 0.999

Repeat the calculation for the value of the K in Part 1b, only this time, do not subtract the [H3O+] from the label con-
a
centration of HAc. How does the value compare to the one you had originally?

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