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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

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter15: Solutions Of Acids And Bases
Section: Chapter Questions
Problem 15.31QE
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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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