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
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![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 104 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;
[A-]
for pH=4.76.
[HA]
[A]
for pH=5.76.
[HA]
[A-]
for pH=8.
Calculate the ratio of;
Calculate the ratio of:
[HA]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d2561ec-5e0b-44bf-843f-c1e0d224382c%2F6dbbcc15-1cfc-4cd1-bdd0-1e742199c23d%2Fmepsa2c_processed.png&w=3840&q=75)
Transcribed Image Text: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 104 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;
[A-]
for pH=4.76.
[HA]
[A]
for pH=5.76.
[HA]
[A-]
for pH=8.
Calculate the ratio of;
Calculate the ratio of:
[HA]
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