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If the bicarbonate ion (HCO3-) concentration in a sample of blood is 0.135 M, determine the carbonic acid (H2CO3) concentration required to buffer the pH of blood at pH = 7.35.               H 2 CO 3(aq)   ⇌ HCO 3 - (aq)  + H + (aq)                                  K a  = 5.3 × 10 -7

If the bicarbonate ion (HCO3-) concentration in a sample of blood is 0.135 M, determine the carbonic acid (H2CO3) concentration required to buffer the pH of blood at pH = 7.35.               H 2 CO 3(aq)   ⇌ HCO 3 - (aq)  + H + (aq)                                  K a  = 5.3 × 10 -7

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
8th Edition
ISBN:9781285199030
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter16: Acids And Bases
Section: Chapter Questions
Problem 42QAP
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If the bicarbonate ion (HCO3-) concentration in a sample of blood is 0.135 M, determine the carbonic acid (H2CO3) concentration required to buffer the pH of blood at pH = 7.35.

              H2CO3(aq)  ⇌  HCO3-(aq) + H+(aq)                                 Ka = 5.3 × 10-7

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