An analytical chemist is titrating 123.4 mL of a 0.2500M solution of propylamine (C3H₂NH₂) with a 0.4100M propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 15.4 mL of the HNO3 se Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the Round your answer to 2 decimal places.

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Chapter16: Acid-base Equilibria
Section: Chapter Questions
Problem 16.113QP: Methylammonium chloride is a salt of methylamine, CH3NH2. A 0.10 M solution of this salt has a pH of...
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An analytical chemist is titrating 123.4 mL of a 0.2500M solution of propylamine (C₂H-NH₂) with a 0.4100M solution of HNO3. The p K, of
propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 15.4 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 = 0
X
S ?
Transcribed Image Text:An analytical chemist is titrating 123.4 mL of a 0.2500M solution of propylamine (C₂H-NH₂) with a 0.4100M solution of HNO3. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 15.4 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 = 0 X S ?
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