An analytical chemist is titrating 236.4 mL of a 0.3500M solution of trimethylamine ((CH₂)¸N)\ with a 0.2300M solution of HNO3. The pK, of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 77.8 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 = 0 X

An analytical chemist is titrating 236.4 mL of a 0.3500M solution of trimethylamine ((CH₂)¸N)\ with a 0.2300M solution of HNO3. The pK, of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 77.8 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 = 0 X

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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