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Consider the titration of 60.00 mL of 0.450 M methylamine (CH3NH2, Kb = 4.4x10^-4) with .600 M hydroiodic acid. What is the pH of this solution when 25.00 mL of titrant is added? What is the pH of this solution when 45.00 mL of titrant have been added?

Consider the titration of 60.00 mL of 0.450 M methylamine (CH3NH2, Kb = 4.4x10^-4) with .600 M hydroiodic acid. What is the pH of this solution when 25.00 mL of titrant is added? What is the pH of this solution when 45.00 mL of titrant have been added?

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria
Section17.3: Acid-base Titrations
Problem 17.6CYU: The titration of 0.100 M acetic acid with 0.100 M NaOH is described in the text. What is the pH of...
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Consider the titration of 60.00 mL of 0.450 M methylamine (CH3NH2, Kb = 4.4x10^-4) with .600 M hydroiodic acid. What is the pH of this solution when 25.00 mL of titrant is added? What is the pH of this solution when 45.00 mL of titrant have been added?
Transcribed Image Text:Consider the titration of 60.00 mL of 0.450 M methylamine (CH3NH2, Kb = 4.4x10^-4) with .600 M hydroiodic acid. What is the pH of this solution when 25.00 mL of titrant is added? What is the pH of this solution when 45.00 mL of titrant have been added?
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