8. Calculate the pH of an aqueous solution containing the following:a. 0.80 M lactic acid and 0.40 M lactate ion(Ka of lactic acid = 1.38 x 104)(Kb of NH3 = 1.8 x 10-5)b. 0.30 M NH3 and 1.50 M NH4+9. Carbonic acid (H2CO3) and bicarbonate ion (HCO3) are used as a buffer system to regulate the bloodpH. An exhausted marathon runner experienced acidosis as his blood pH become 7.15. What is the ratioof HCO3 to H2CO3 in this pH? (Ka of H2CO3 = 4.2 x 10-7)

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8. Calculate the pH of an aqueous solution containing the following: a. 0.80 M lactic acid and 0.40 M lactate ion b. 0.30 M NH3 and 1.50 M NH4+ (Ka of lactic acid 1.38 x 104) (Kb of NH3 = 1.8 x 10-5)

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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Question

8. Calculate the pH of an aqueous solution containing the following:
a. 0.80 M lactic acid and 0.40 M lactate ion
(Ka of lactic acid = 1.38 x 104)
(Kb of NH3 = 1.8 x 10-5)
b. 0.30 M NH3 and 1.50 M NH4+
9. Carbonic acid (H2CO3) and bicarbonate ion (HCO3) are used as a buffer system to regulate the blood
pH. An exhausted marathon runner experienced acidosis as his blood pH become 7.15. What is the ratio
of HCO3 to H2CO3 in this pH? (Ka of H2CO3 = 4.2 x 10-7)

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