Consider the titration of 50.0 mL of 0.309 M B (weak base, Kb =7.5 x 106) with 0.340 M HNO3. What is the pH of the solution after the addition of: - 90.0 mL of HNO₂? - 45.44 mL of HNO3? 0.0 mL of HNO3?
Consider the titration of 50.0 mL of 0.309 M B (weak base, Kb =7.5 x 106) with 0.340 M HNO3. What is the pH of the solution after the addition of: - 90.0 mL of HNO₂? - 45.44 mL of HNO3? 0.0 mL of HNO3?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter15: Acid-base Equilibria
Section: Chapter Questions
Problem 65E: Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 105) by 0.100 M KOH. Calculate...
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![Consider the titration of 50.0 mL of 0.309 M B (weak
base, Kb =7.5 x 10-6) with 0.340 M HNO3.
What is the pH of the solution after the addition of:
- 90.0 mL of HNO₂?
- 45.44 mL of HNO3?
- 0.0 mL of HNO3?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F79338ae7-95ae-4aeb-b3b3-7c1af94b0a9e%2F6d68a56d-9c72-49fd-9b93-b1d3c4bc7569%2F4xmqhko_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Consider the titration of 50.0 mL of 0.309 M B (weak
base, Kb =7.5 x 10-6) with 0.340 M HNO3.
What is the pH of the solution after the addition of:
- 90.0 mL of HNO₂?
- 45.44 mL of HNO3?
- 0.0 mL of HNO3?
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