Consider the titration of 60.0 mL of 0.0400 M (CH3)2NH (a weak base; K = 0.000540) with 0.100 M HBrO 4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = (d) 18.0 mL pH = (b) 6.0 mL pH = (e) 24.0 mL pH = (c) 12.0 mL pH = (f) 43.2 mL pH =
Consider the titration of 60.0 mL of 0.0400 M (CH3)2NH (a weak base; K = 0.000540) with 0.100 M HBrO 4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = (d) 18.0 mL pH = (b) 6.0 mL pH = (e) 24.0 mL pH = (c) 12.0 mL pH = (f) 43.2 mL pH =
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter15: Additional Aqueous Equilibria
Section: Chapter Questions
Problem 34QRT
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![Consider the titration of 60.0 mL of 0.0400 M (CH3)2NH (a weak base; K₁ = 0.000540) with 0.100 M HBrO4. Calculate the
pH after the following volumes of titrant have been added:
(a) 0.0 mL
PH
(d) 18.0 mL
PH =
(b) 6.0 mL
pH =
(e) 24.0 mL
pH =
(c) 12.0 mL
pH =
(f) 43.2 mL
pH =](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F86624ab7-da2a-4a5b-91b8-0bf4ad8ab366%2F7c3d8fea-01fd-432a-8b87-f3201b909bd4%2F4yovuv_processed.png&w=3840&q=75)
Transcribed Image Text:Consider the titration of 60.0 mL of 0.0400 M (CH3)2NH (a weak base; K₁ = 0.000540) with 0.100 M HBrO4. Calculate the
pH after the following volumes of titrant have been added:
(a) 0.0 mL
PH
(d) 18.0 mL
PH =
(b) 6.0 mL
pH =
(e) 24.0 mL
pH =
(c) 12.0 mL
pH =
(f) 43.2 mL
pH =
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