141480 4. A student needs to prepare a buffer solution with a pH of 5.59. Assuming a pka of 4.54, how many mL of 0.1 M NaOH would need to be added to 24.0 mL of 0.1 M HB to prepare this buffer? Please include a proper (abbreviated) unit. HINT: Use pH = pKa + log ([B-]/[HB]) or, if concentrations are the same, pH = pka + log (Volume of OH-/ (Volume of HB - Volume of OH-) mis
141480 4. A student needs to prepare a buffer solution with a pH of 5.59. Assuming a pka of 4.54, how many mL of 0.1 M NaOH would need to be added to 24.0 mL of 0.1 M HB to prepare this buffer? Please include a proper (abbreviated) unit. HINT: Use pH = pKa + log ([B-]/[HB]) or, if concentrations are the same, pH = pka + log (Volume of OH-/ (Volume of HB - Volume of OH-) mis
Chemistry
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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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![4. A student needs to prepare a buffer solution with a pH of 5.59. Assuming a pka of 4.54,
how many mL of 0.1 M NaOH would need to be added to 24.0 mL of 0.1 M HB to
prepare this buffer? Please include a proper (abbreviated) unit.
HINT: Use pH = pKa + log ([B-]/[HB]) or, if concentrations are the same,
pH = pka + log (Volume of OH-/ (Volume of HB - Volume of OH-)
olved.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc2879e7b-b9eb-4caf-a2bf-32a860571f77%2F6ceb4cc9-9a99-453d-96ae-921ae4b711fb%2Fic4yqww_processed.jpeg&w=3840&q=75)
Transcribed Image Text:4. A student needs to prepare a buffer solution with a pH of 5.59. Assuming a pka of 4.54,
how many mL of 0.1 M NaOH would need to be added to 24.0 mL of 0.1 M HB to
prepare this buffer? Please include a proper (abbreviated) unit.
HINT: Use pH = pKa + log ([B-]/[HB]) or, if concentrations are the same,
pH = pka + log (Volume of OH-/ (Volume of HB - Volume of OH-)
olved.
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