Calculating the pH of a weak base titrated with a strong acid An analytical chemist is titrating 112.5 mL of a 0.1400M solution of dimethylamine ((CH3)2NH) with a 0.2800 M solution of HNO3. The pK, of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 64.5 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 = 3/5 Izabella 000
Calculating the pH of a weak base titrated with a strong acid An analytical chemist is titrating 112.5 mL of a 0.1400M solution of dimethylamine ((CH3)2NH) with a 0.2800 M solution of HNO3. The pK, of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 64.5 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 = 3/5 Izabella 000
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter14: Acid-base Equilibria
Section: Chapter Questions
Problem 115E: Calculate the pH at the following points in a titration of 40 mL (0.040 L) of 0.100 M barbituric...
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