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
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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