Use the HH equation to solve for the ratio of conjugate base to weak acid at pH=1. The pKa of acetic acid is 4.76. [A-) 1 = 4.76 + log| [HA], = 1.7 x 10-4 [HA] This is really a ratio, meaning that at pH 1, there is 1.7 x 10-4 mol A¯ for every 1 mol HA. The buffer is very far out of equilibrium. This is why the titration curve rises so sharply in this pH range. • Use the HH equation to solve for the ratio of conjugate base to weak acid at pH=3.76. • Calculate the ratio of: for pH=4.76. [HA] Calculate the ratio of; for pH=5.76. [HA] • Calculate the ratio of for pH=8. [HA]

Use the HH equation to solve for the ratio of conjugate base to weak acid at pH=1. The pKa of acetic acid is 4.76. [A-) 1 = 4.76 + log| [HA], = 1.7 x 10-4 [HA] This is really a ratio, meaning that at pH 1, there is 1.7 x 10-4 mol A¯ for every 1 mol HA. The buffer is very far out of equilibrium. This is why the titration curve rises so sharply in this pH range. • Use the HH equation to solve for the ratio of conjugate base to weak acid at pH=3.76. • Calculate the ratio of: for pH=4.76. [HA] Calculate the ratio of; for pH=5.76. [HA] • Calculate the ratio of for pH=8. [HA]

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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Buffers will resist pH changes following the addition of acid or base within about +/-1 pH unit of the pka of a solution. True False
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