The pH of blood plasma is 7.40. Assuming that the principal buffer system in blood is HCO, /H2CO3, A) determine the ratio [HCO,]/[H¿CO3] in blood plasma. The ionization con- stant of carbonic acid is K.(H2CO3) = 4.3 x 10-7. B) Based on your result in part (A), how many moles of H2CO3 (assuming that they occupy no volume) would need to be added to 300.0 mL of an aqueous solution that is 0.250 mol L- in NaHCOz to make a buffer solution of the same pH as blood plasma? To solve the problem you may assume that the solutions behave as ideal dilute solutions (solute-type activity coefficients equal to unity).
The pH of blood plasma is 7.40. Assuming that the principal buffer system in blood is HCO, /H2CO3, A) determine the ratio [HCO,]/[H¿CO3] in blood plasma. The ionization con- stant of carbonic acid is K.(H2CO3) = 4.3 x 10-7. B) Based on your result in part (A), how many moles of H2CO3 (assuming that they occupy no volume) would need to be added to 300.0 mL of an aqueous solution that is 0.250 mol L- in NaHCOz to make a buffer solution of the same pH as blood plasma? To solve the problem you may assume that the solutions behave as ideal dilute solutions (solute-type activity coefficients equal to unity).
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
Chapter15: Acid-base Equilibria
Section: Chapter Questions
Problem 2ALQ: A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt...
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![The pH of blood plasma is 7.40. Assuming that the principal buffer system in blood
is HCO, /H2CO3,
A) determine the ratio [HCO,]/[H2CO3] in blood plasma. The ionization con-
stant of carbonic acid is K.(H2CO3) = 4.3 x 10-7.
B) Based on your result in part (A), how many moles of H2CO3 (assuming
that they occupy no volume) would need to be added to 300.0 mL of
an aqueous solution that is 0.250 mol L- in NaHCO3 to make a buffer
solution of the same pH as blood plasma?
To solve the problem you may assume that the solutions behave as ideal dilute solutions
(solute-type activity coefficients equal to unity).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F12958458-96f4-4f8c-8330-c5f03483b490%2Fc0ed4764-1efe-4e32-bf5c-c5eb8aed4e6e%2Fvy65f48_processed.png&w=3840&q=75)
Transcribed Image Text:The pH of blood plasma is 7.40. Assuming that the principal buffer system in blood
is HCO, /H2CO3,
A) determine the ratio [HCO,]/[H2CO3] in blood plasma. The ionization con-
stant of carbonic acid is K.(H2CO3) = 4.3 x 10-7.
B) Based on your result in part (A), how many moles of H2CO3 (assuming
that they occupy no volume) would need to be added to 300.0 mL of
an aqueous solution that is 0.250 mol L- in NaHCO3 to make a buffer
solution of the same pH as blood plasma?
To solve the problem you may assume that the solutions behave as ideal dilute solutions
(solute-type activity coefficients equal to unity).
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