An analytical chemist is titrating 173.4 mL of a 0.6400 M solution of trimethylamine ((CH,) N with a 0.8100 M solution of HNO3. The p K, of 3 trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 59.0 mL of the HNO, solution to it. 3. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.

An analytical chemist is titrating 173.4 mL of a 0.6400 M solution of trimethylamine ((CH,) N with a 0.8100 M solution of HNO3. The p K, of 3 trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 59.0 mL of the HNO, solution to it. 3. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 26QAP: You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio...

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