You have 30.00 mL of a 0.250 M aqueous solution of the weak base (CH3)2NH (Kb= 7.40 x 10-4). This solution will be titrated with 0.250 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 5.00 mL of acid has been added? (d) What is the pH of the solution at the equivalence point of the titration? (e) What is the pH of the solution when 35.00 mL of acid has been added?
You have 30.00 mL of a 0.250 M aqueous solution of the weak base (CH3)2NH (Kb= 7.40 x 10-4). This solution will be titrated with 0.250 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 5.00 mL of acid has been added? (d) What is the pH of the solution at the equivalence point of the titration? (e) What is the pH of the solution when 35.00 mL of acid has been added?
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 47QAP: A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide. (Assume...
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You have 30.00 mL of a 0.250 M aqueous solution of the weak base (CH3)2NH (Kb= 7.40 x 10-4).
This solution will be titrated with 0.250 M HCl.
(a) How many mL of acid must be added to reach the equivalence point?
(b) What is the pH of the solution before any acid is added?
(c) What is the pH of the solution after 5.00 mL of acid has been added?
(d) What is the pH of the solution at the equivalence point of the titration?
(e) What is the pH of the solution when 35.00 mL of acid has been added?
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