An analytical chemist is titrating 168.4 mL of a 0.2500 M solution of ammonia (NH,) with a 0.7000 M solution of HNO3. The p Kh of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 71.9 mL of the HNO, solution to it. 3 Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = 0
An analytical chemist is titrating 168.4 mL of a 0.2500 M solution of ammonia (NH,) with a 0.7000 M solution of HNO3. The p Kh of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 71.9 mL of the HNO, solution to it. 3 Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = 0
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
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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![An analytical chemist is titrating 168.4 mL of a 0.2500 M solution of ammonia (NH,) with a 0.7000 M solution of HNO3. The p Kh of ammonia is 4.74.
Calculate the pH of the base solution after the chemist has added 71.9 mL of the HNO, solution to it.
3
Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added.
Round your answer to 2 decimal places.
pH = 0](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1a6c4f25-80b7-4e94-8b7d-fa43f07e3fca%2Fc70131e6-dd1a-4f99-9a47-d8314e291430%2F3lnkpq8.jpeg&w=3840&q=75)
Transcribed Image Text:An analytical chemist is titrating 168.4 mL of a 0.2500 M solution of ammonia (NH,) with a 0.7000 M solution of HNO3. The p Kh of ammonia is 4.74.
Calculate the pH of the base solution after the chemist has added 71.9 mL of the HNO, solution to it.
3
Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added.
Round your answer to 2 decimal places.
pH = 0
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