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)

Answered: 8. Calculate the pH of an aqueous…

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: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 179CP: Consider 1000. mL of a 1.00 104-M solution of a certain acid HA that has a Ka value equal to 1.00 ...

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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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