A chemist titrates 50.0 mL of a 0.4629 Methylamine (C₂H-NH₂) solution with 0.1652 MHNO3 solution at 25 °C. Calculate the pH at equivalence. The pK, of ethylamine is 3.19. 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 HNO3 solution added. pH = 0 X Ś
A chemist titrates 50.0 mL of a 0.4629 Methylamine (C₂H-NH₂) solution with 0.1652 MHNO3 solution at 25 °C. Calculate the pH at equivalence. The pK, of ethylamine is 3.19. 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 HNO3 solution added. pH = 0 X Ś
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter15: Acid–base Equilibria
Section: Chapter Questions
Problem 55P
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![A chemist titrates 50.0 mL of a 0.4629 Methylamine (C₂H-NH₂) solution with 0.1652 MHNO3 solution at 25 °C. Calculate the pH at equivalence. The pK, of
ethylamine is 3.19.
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 HNO3 solution added.
pH = 0
X
Ś](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F24823098-9e78-4458-9f4a-747264229ccb%2F7d2e9983-b239-4a92-bdd7-dbabf92c54dd%2Fzt53k7_processed.png&w=3840&q=75)
Transcribed Image Text:A chemist titrates 50.0 mL of a 0.4629 Methylamine (C₂H-NH₂) solution with 0.1652 MHNO3 solution at 25 °C. Calculate the pH at equivalence. The pK, of
ethylamine is 3.19.
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 HNO3 solution added.
pH = 0
X
Ś
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