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¯.
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.113QP: Methylammonium chloride is a salt of methylamine, CH3NH2. A 0.10 M solution of this salt has a pH of...
Related questions
Question
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>
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:
9781285869759
Author:
Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning