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
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Author:William L. Masterton, Cecile N. Hurley
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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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![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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F130d76d2-67f2-4705-be14-2a465b37b9af%2F1699e0a5-15d3-43a2-9f6b-a332f83ce38f%2Fkbd2sk.png&w=3840&q=75)
Transcribed Image Text: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.
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