Consider the titration of 60.0 mL of 0.0400 M (CH3)2NH (a weak base; K = 0.000540) with 0.100 M HBrO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = 11.64 (d) 18.0 mL pH = 10.25 (b) 6.0 mL pH = 11.21 (e) 24.0 mL pH = X (c) 12.0 mL pH = 10.73 (f) 43.2 mL pH = X

Consider the titration of 60.0 mL of 0.0400 M (CH3)2NH (a weak base; K = 0.000540) with 0.100 M HBrO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = 11.64 (d) 18.0 mL pH = 10.25 (b) 6.0 mL pH = 11.21 (e) 24.0 mL pH = X (c) 12.0 mL pH = 10.73 (f) 43.2 mL pH = X

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 66E: In the titration of 50.0 mL of 1.0 M methylamine, CH3NH2 (Kb = 4.4 104), with 0.50 M HC1, calculate...

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