An analytical chemist is titrating 189.5 mL of a 0.6500M solution of ammonia (NH,) with a 0.8000M solution of HNO3. The p K, of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 177.1 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 = 0 alo
An analytical chemist is titrating 189.5 mL of a 0.6500M solution of ammonia (NH,) with a 0.8000M solution of HNO3. The p K, of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 177.1 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 = 0 alo
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 97AE: A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution...
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