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: 0.200 mol CICH, CO, H, 0.080 mol CICH.CO.Na. 0.060 mol HNO,, and 0.060 mol Ca(OH)₂. Ca(OH), provides 2OH". pH =
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: 0.200 mol CICH, CO, H, 0.080 mol CICH.CO.Na. 0.060 mol HNO,, and 0.060 mol Ca(OH)₂. Ca(OH), provides 2OH". pH =
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter16: Reactions Between Acids And Bases
Section: Chapter Questions
Problem 16.80QE: Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus...
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![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: 0.200 mol CICH, CO, H, 0.080 mol CICH,CO,Na,
0.060 mol HNO,, and 0.060 mol Ca(OH)₂. Ca(OH), provides 2OH™.
pH =](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe51f4502-266c-4a2e-9961-b5c5485019ee%2Fdfa112ae-b35e-4bfc-8410-23c953ed56b6%2Fotiy0s6_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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: 0.200 mol CICH, CO, H, 0.080 mol CICH,CO,Na,
0.060 mol HNO,, and 0.060 mol Ca(OH)₂. Ca(OH), provides 2OH™.
pH =
![Calculate the pH of a solution prepared by mixing 0.0740 mol of chloroacetic acid plus 0.0240 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 pK, of
chloroacetic acid is 2.865.
pH =
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 =
-](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe51f4502-266c-4a2e-9961-b5c5485019ee%2Fdfa112ae-b35e-4bfc-8410-23c953ed56b6%2Fpfowpmn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Calculate the pH of a solution prepared by mixing 0.0740 mol of chloroacetic acid plus 0.0240 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 pK, of
chloroacetic acid is 2.865.
pH =
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 =
-
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