An analytical chemist is titrating 187.6 mL of a 0.4000M solution of trimethylamine ((CH3),N) with a 0.7000M solution of HNO2. The p K, of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 19.8 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO2 solution added. Round your answer to 2 decimal places. pH =

An analytical chemist is titrating 187.6 mL of a 0.4000M solution of trimethylamine ((CH3),N) with a 0.7000M solution of HNO2. The p K, of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 19.8 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO2 solution added. Round your answer to 2 decimal places. pH =

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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