An analytical chemist is titrating 131.8 mL of a 0.7000M solution of propylamine (C3H-NH₂) with a 0.7800M solution of HNO3. The p K₂ of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 126.1 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.

An analytical chemist is titrating 131.8 mL of a 0.7000M solution of propylamine (C3H-NH₂) with a 0.7800M solution of HNO3. The p K₂ of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 126.1 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.

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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