10⁻⁸) with 0.100 M LiOH. a) What is the pH of the solution before any base has been added? b) What would be the pH of the solution after the addition of 20.0 mL of LiOH? c) How many mL of the LiOH would be required to reach the halfway point of the titration?
10⁻⁸) with 0.100 M LiOH. a) What is the pH of the solution before any base has been added? b) What would be the pH of the solution after the addition of 20.0 mL of LiOH? c) How many mL of the LiOH would be required to reach the halfway point of the titration?
General Chemistry - Standalone book (MindTap Course List)
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.148QP
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Question
1. Consider the titration of a 40.0 mL of 0.193 M weak acid HA (Ka = 2.7 x 10⁻⁸) with 0.100 M LiOH.
a) What is the pH of the solution before any base has been added?
b) What would be the pH of the solution after the addition of 20.0 mL of LiOH?
c) How many mL of the LiOH would be required to reach the halfway point of the titration?
d) What is the pH of the solution at the equivalence point?
e) What would be the pH of the solution after that addition of 100.0 mL of LiOH?
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