6. A 100 mL sample of 0.13 M trimethylamine, (CH3)3N, aqueous solution is titrated with 0.31 M HCI solution at 25 °C. Kb for (CH3)3N = 6.4 x 10-5. a. Calculate the pH of the solution after 25 mL of HCl solution has been added. b. How many mL of 0.31 M HCI need to be added to the sample to reach the equivalence point? What is the pH at the equivalence point?

6. A 100 mL sample of 0.13 M trimethylamine, (CH3)3N, aqueous solution is titrated with 0.31 M HCI solution at 25 °C. Kb for (CH3)3N = 6.4 x 10-5. a. Calculate the pH of the solution after 25 mL of HCl solution has been added. b. How many mL of 0.31 M HCI need to be added to the sample to reach the equivalence point? What is the pH at the equivalence point?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 59E: Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 105) by 0.100 M KOH. Calculate...

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