A student needs to prepare a buffer solution with a pH of 4.21. Assuming a pK, of 4.15, how many mL of 0.1 M B¯ would need to be added to 22.0 mL of 0.1 M HB prepare this buffer? Please include a proper (abbreviated) unit. HINT : Use pH = pKa + log ([B minus]/[HB]) or, if %3D concentrations are the same, pH = pka + log (Volume of B minus/ Volume of HB) %D
A student needs to prepare a buffer solution with a pH of 4.21. Assuming a pK, of 4.15, how many mL of 0.1 M B¯ would need to be added to 22.0 mL of 0.1 M HB prepare this buffer? Please include a proper (abbreviated) unit. HINT : Use pH = pKa + log ([B minus]/[HB]) or, if %3D concentrations are the same, pH = pka + log (Volume of B minus/ Volume of HB) %D
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 16.142QP: K4 for acetic acid is 1.7 105 at 25C. A buffer solution is made by mixing 52.1 mL of 0.122 M acetic...
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![A student needs to prepare a buffer solution
with a pH of 4.21. Assuming a pK, of 4.15, how
many ml of 0.1 M B¯ would need to be added
to 22.0 mL of 0.1 M HB prepare this buffer?
Please include a proper (abbreviated) unit.
HINT : Use pH = pK, + log ([B minus]/[HB]) or, if
%3D
concentrations are the same,
pH = pka + log (Volume of B minus/ Volume of
%3D
HB)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3f7858f2-4558-4a97-afcd-256e507c1a66%2F62750b7f-cd1d-49a0-b506-7e2e61046242%2Fqsgiqag_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A student needs to prepare a buffer solution
with a pH of 4.21. Assuming a pK, of 4.15, how
many ml of 0.1 M B¯ would need to be added
to 22.0 mL of 0.1 M HB prepare this buffer?
Please include a proper (abbreviated) unit.
HINT : Use pH = pK, + log ([B minus]/[HB]) or, if
%3D
concentrations are the same,
pH = pka + log (Volume of B minus/ Volume of
%3D
HB)
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