Carbonic acid (H2CO3) is a weak acid and is therefore in equilibrium with bicarbonate (HCO3-) in solution. When significant amounts of both carbonic acid and bicarbonate are present, a buffer is formed. This buffer system can be written as: H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) If the carbonic acid (H2CO3) concentration in a sample of blood is 0.00125 M, determine the bicarbonate ion (HCO3-) concentration required to buffer the pH of blood at pH = 7.40. H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) Ka = 4.3 × 10-7 Show all calculations including equation(s) used.
Carbonic acid (H2CO3) is a weak acid and is therefore in equilibrium with bicarbonate (HCO3-) in solution. When significant amounts of both carbonic acid and bicarbonate are present, a buffer is formed. This buffer system can be written as: H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) If the carbonic acid (H2CO3) concentration in a sample of blood is 0.00125 M, determine the bicarbonate ion (HCO3-) concentration required to buffer the pH of blood at pH = 7.40. H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) Ka = 4.3 × 10-7 Show all calculations including equation(s) used.
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Carbonic acid (H2CO3) is a weak acid and is therefore in equilibrium with bicarbonate (HCO3-) in solution. When significant amounts of both carbonic acid and bicarbonate are present, a buffer is formed. This buffer system can be written as: H2CO3(aq) ⇌ HCO3-(aq) + H+(aq)
If the carbonic acid (H2CO3) concentration in a sample of blood is 0.00125 M, determine the bicarbonate ion (HCO3-) concentration required to buffer the pH of blood at pH = 7.40.
H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) Ka = 4.3 × 10-7
Show all calculations including equation(s) used.
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