An analytical chemist is titrating 112.7 mL of a 0.6400M solution of ethylamine (C₂H5NH₂) with a 0.8100M solution of HNO3. The p K, of ethylamine is 3.19. Calculate the pH of the base solution after the chemist has added 21.5 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 112.7 mL of a 0.6400M solution of ethylamine (C₂H5NH₂) with a 0.8100M solution of HNO3. The p K, of ethylamine is 3.19. Calculate the pH of the base solution after the chemist has added 21.5 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.

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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