Calculate the pH of a solution prepared by mixing 0.0730 mol of chloroacetic acid plus 0.0140 mol of sodium chloroacetate in 1.00 L of water. First do the calculation by assuming that the concentrations of HA and A equal their formal concentrations. The pKa of chloroacetic acid is 2.865. pH = 2.15 Then do the calculation with [HA] and [A¯] from Equations 9-21 and 9-22. [HA] = FHA [H*]+ [OH¯] (9-21) [A¯] = FA- + [H*] - [OH¯] (9-22) pH = 2.865 Using first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all the following compounds in one beaker containing a total volume of 1.00 L: 0.170 mol CICH, CO,H, 0.050 mol CICH,CO,Na, 0.060 mol HNO,, and 0.060 mol Ca(OH), . Ca(OH), provides 2 OH¯.
Calculate the pH of a solution prepared by mixing 0.0730 mol of chloroacetic acid plus 0.0140 mol of sodium chloroacetate in 1.00 L of water. First do the calculation by assuming that the concentrations of HA and A equal their formal concentrations. The pKa of chloroacetic acid is 2.865. pH = 2.15 Then do the calculation with [HA] and [A¯] from Equations 9-21 and 9-22. [HA] = FHA [H*]+ [OH¯] (9-21) [A¯] = FA- + [H*] - [OH¯] (9-22) pH = 2.865 Using first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all the following compounds in one beaker containing a total volume of 1.00 L: 0.170 mol CICH, CO,H, 0.050 mol CICH,CO,Na, 0.060 mol HNO,, and 0.060 mol Ca(OH), . Ca(OH), provides 2 OH¯.
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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Please answer all 3 parts.
![Calculate the pH of a solution prepared by mixing 0.0730 mol of chloroacetic acid plus 0.0140 mol of sodium chloroacetate
in 1.00 L of water.
First do the calculation by assuming that the concentrations of HA and A equal their formal concentrations. The pKa of
chloroacetic acid is 2.865.
pH =
2.15
Then do the calculation with [HA] and [A¯] from Equations 9-21 and 9-22.
[HA] = FHA - [H*]+ [OH¯]
(9-21)
[A-] = FA- + [H*]- [OH¯]
(9-22)
pH =
2.865
Using first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all the
following compounds in one beaker containing a total volume of 1.00 L: 0.170 mol CICH, CO, H, 0.050 mol CICH, CO,Na,
0.060 mol HNO,, and 0.060 mol Ca(OH), . Ca(OH), provides 2 OH-.
3>](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F66f02499-6a2e-4c33-a9a6-3b6555c8b394%2Fb03453fe-8822-4b39-9496-2f0833bd2b61%2Fsfks39j_processed.png&w=3840&q=75)
Transcribed Image Text:Calculate the pH of a solution prepared by mixing 0.0730 mol of chloroacetic acid plus 0.0140 mol of sodium chloroacetate
in 1.00 L of water.
First do the calculation by assuming that the concentrations of HA and A equal their formal concentrations. The pKa of
chloroacetic acid is 2.865.
pH =
2.15
Then do the calculation with [HA] and [A¯] from Equations 9-21 and 9-22.
[HA] = FHA - [H*]+ [OH¯]
(9-21)
[A-] = FA- + [H*]- [OH¯]
(9-22)
pH =
2.865
Using first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all the
following compounds in one beaker containing a total volume of 1.00 L: 0.170 mol CICH, CO, H, 0.050 mol CICH, CO,Na,
0.060 mol HNO,, and 0.060 mol Ca(OH), . Ca(OH), provides 2 OH-.
3>
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