Consider the titration of 30.0 mL of 0.271 M weak base B (Kb = 1.3 x 10⁻¹⁰) with 0.150 M HI. b. What would be the pH of the solution after the addition of 20.0 mL of HI? d. What is the pH of the solution at the equivalence point? e. What would be the pH of the solution after the addition of 100.0 mL of HI?
Consider the titration of 30.0 mL of 0.271 M weak base B (Kb = 1.3 x 10⁻¹⁰) with 0.150 M HI. b. What would be the pH of the solution after the addition of 20.0 mL of HI? d. What is the pH of the solution at the equivalence point? e. What would be the pH of the solution after the addition of 100.0 mL of HI?
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter14: Acid- Base Equilibria
Section: Chapter Questions
Problem 106CWP: Consider the titration of 100.0 mL of 0.200 M HONH2 by 0.100 M HCI. (Kb for HONH2 = 1.1 108.) a....
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Consider the titration of 30.0 mL of 0.271 M weak base B (Kb = 1.3 x 10⁻¹⁰) with 0.150 M HI.
b. What would be the pH of the solution after the addition of 20.0 mL of HI?
d. What is the pH of the solution at the equivalence point?
e. What would be the pH of the solution after the addition of 100.0 mL of HI?
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