An analytical chemist is titrating 200.4 mL of a 0.6100M solution of methylamine (CH3NH2) with a 0.5100M solution of HNO3. The pK of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 86.9 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = X Ś الله Ar
An analytical chemist is titrating 200.4 mL of a 0.6100M solution of methylamine (CH3NH2) with a 0.5100M solution of HNO3. The pK of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 86.9 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = X Ś الله Ar
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.113QP: Methylammonium chloride is a salt of methylamine, CH3NH2. A 0.10 M solution of this salt has a pH of...
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![An analytical chemist is titrating 200.4 mL of a 0.6100M solution of methylamine (CH3NH2) with a 0.5100M solution of HNO3. The pK of methylamine is
3.36. Calculate the pH of the base solution after the chemist has added 86.9 mL of the HNO3 solution to it.
Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added.
Round your answer to 2 decimal places.
pH =
X
Ś
الله
Ar](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F39b87e10-904d-437c-ab82-c08b3982d249%2F791266ec-d8ee-4bdd-9b9e-1928526886bc%2F5xqzqu_processed.jpeg&w=3840&q=75)
Transcribed Image Text:An analytical chemist is titrating 200.4 mL of a 0.6100M solution of methylamine (CH3NH2) with a 0.5100M solution of HNO3. The pK of methylamine is
3.36. Calculate the pH of the base solution after the chemist has added 86.9 mL of the HNO3 solution to it.
Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added.
Round your answer to 2 decimal places.
pH =
X
Ś
الله
Ar
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