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2. Carbonic acid (H₂CO3) and bicarbonate (HCO3) act as buffers in the blood. (a) What is the origin of carbonic acid? (b) Write the equilibrium equation for dissociation of carbonic acid in water to give bicarbonate and hydronium ions. (c) Typical concentrations of carbonic acid and bicarbonate are 0.0024 M and 0.024 M, respectively. Calculate the pH of blood. (K, of carbonic acid = 4.3 x 10-7)

2. Carbonic acid (H₂CO3) and bicarbonate (HCO3) act as buffers in the blood. (a) What is the origin of carbonic acid? (b) Write the equilibrium equation for dissociation of carbonic acid in water to give bicarbonate and hydronium ions. (c) Typical concentrations of carbonic acid and bicarbonate are 0.0024 M and 0.024 M, respectively. Calculate the pH of blood. (K, of carbonic acid = 4.3 x 10-7)

Chemistry
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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2. Carbonic acid (H₂CO3) and bicarbonate (HCO3) act as buffers in the blood. (a) What is the origin of carbonic acid? (b) Write the equilibrium equation for dissociation of carbonic acid in water to give bicarbonate and hydronium ions. (c) Typical concentrations of carbonic acid and bicarbonate are 0.0024 M and 0.024 M, respectively. Calculate the pH of blood. (K, of carbonic acid = 4.3 x 10-7)
Transcribed Image Text:2. Carbonic acid (H₂CO3) and bicarbonate (HCO3) act as buffers in the blood. (a) What is the origin of carbonic acid? (b) Write the equilibrium equation for dissociation of carbonic acid in water to give bicarbonate and hydronium ions. (c) Typical concentrations of carbonic acid and bicarbonate are 0.0024 M and 0.024 M, respectively. Calculate the pH of blood. (K, of carbonic acid = 4.3 x 10-7)
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