An analytical chemist is titrating 74.2 mL of a 0.3000 M solution of methylamine (CH3NH2) with a 0.2500M solution of HNO3. The pK of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 10.4 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. PH = ☐
An analytical chemist is titrating 74.2 mL of a 0.3000 M solution of methylamine (CH3NH2) with a 0.2500M solution of HNO3. The pK of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 10.4 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. PH = ☐
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 16.131QP: A quantity of 0.25 M sodium hydroxide is added to a solution containing 0.15 mol of acetic acid. The...
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