1. Acetic acid is a weak monoprotic acid with Ka = 1.77 x 10¯5. NaOH(s) was gradually added to 1.00 L of 0.0179 M acetic acid. (Assume no volume change occurs.) Calculate the pH of the solution after the addition of 0.0286 mol of NaOH(s). A. 8.502 B. 1.971 C. 12.029 D. 7.0002.What is the ratio of [A-] / [HA] for a buffer solution of HA with a pH of 7 if the pKa = 5 for HA? A. 100 B. 0.01 C. 10 D. 0.13. Titrate 50.0 ml 0.1 M HCN (Ka = 6.2 x 10-10) with 0.10 M NaOH. Calculate the pH at the half-way or midpoint. A. 9.2 B. 7.0 C. 4.8 D. 0.0

The Henderson-Hasselbalch equation for the acidic buffer solution is: pH=pKa+logA-HA ......(1)

Answered: 1. Acetic acid is a weak monoprotic…

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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1. Acetic acid is a weak monoprotic acid with K_a = 1.77 x 10¯⁵. NaOH(s) was gradually added to 1.00 L of 0.0179 M acetic acid. (Assume no volume change occurs.) Calculate the pH of the solution after the addition of 0.0286 mol of NaOH(s).

A.
8.502
B.
1.971
C.
12.029
D.
7.000

2.What is the ratio of [A^-] / [HA] for a buffer solution of HA with a pH of 7 if the pK_a = 5 for HA?

A.
100
B.
0.01
C.
10
D.
0.1

Titrate 50.0 ml 0.1 M HCN (Ka = 6.2 x 10^-10) with 0.10 M NaOH. Calculate the pH at the half-way or midpoint.

A.
9.2
B.
7.0
C.
4.8
D.
0.0

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