An analytical chemist is titrating 150.6 mL of a 0.4500 M solution of ammonia (NH,) with a 0.6900 M solution of HNO2. The p K, of ammonia is 4.74. 3 Calculate the pH of the base solution after the chemist has added 113.8 mL of the HNO, solution to it. 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 %3D
An analytical chemist is titrating 150.6 mL of a 0.4500 M solution of ammonia (NH,) with a 0.6900 M solution of HNO2. The p K, of ammonia is 4.74. 3 Calculate the pH of the base solution after the chemist has added 113.8 mL of the HNO, solution to it. 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 %3D
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 150.6 mL of a 0.4500 M solution of ammonia (NH,) with a 0.6900 M solution of HNO2. The p K, of ammonia is 4.74.
3
Calculate the pH of the base solution after the chemist has added 113.8 mL of the HNO, solution to it.
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
%3D](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdfa4dcdb-77f6-4ef0-bc13-c2ab2b3645e1%2Fadd35fad-faec-4681-bb68-57d19f3ba4d8%2F6o14lm8.jpeg&w=3840&q=75)
Transcribed Image Text:An analytical chemist is titrating 150.6 mL of a 0.4500 M solution of ammonia (NH,) with a 0.6900 M solution of HNO2. The p K, of ammonia is 4.74.
3
Calculate the pH of the base solution after the chemist has added 113.8 mL of the HNO, solution to it.
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
%3D
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