A chemist titrates 110.0 mL of a 0.2187M trimethylamine ((CH3)¸N) ³ N) solution with 0.8123 M HCl solution at 25 °C. Calculate the pH at equivalence. The p K of trimethylamine is 4.19.
A chemist titrates 110.0 mL of a 0.2187M trimethylamine ((CH3)¸N) ³ N) solution with 0.8123 M HCl solution at 25 °C. Calculate the pH at equivalence. The p K of trimethylamine is 4.19.
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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The answer is not 5.45
![A chemist titrates 110.0 mL of a 0.2187M trimethylamine ((CH3)N)
of trimethylamine is 4.19.
N) solution with 0.8123 M HCl solution at 25 °C. Calculate the pH at equivalence. The p K
Round your answer to 2 decimal places.
Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcdb4ed13-3d7d-46b8-a9c5-32c3c2750547%2F3210f1c0-b0c9-4bc6-9d80-4b37a3ee0b85%2F1jje1lf_processed.png&w=3840&q=75)
Transcribed Image Text:A chemist titrates 110.0 mL of a 0.2187M trimethylamine ((CH3)N)
of trimethylamine is 4.19.
N) solution with 0.8123 M HCl solution at 25 °C. Calculate the pH at equivalence. The p K
Round your answer to 2 decimal places.
Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added.
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