A solution of methylamine, CH3NH2, behaves as a weak base. The equilibrium can be written as: CH3NH₂ + H+ = [CH3NH3]+ Methylamine has Kb = = 4.6 x 10-4. a) Calculate the pH of a methylamine solution with a concentration of 0.25 mol dm-³. 60.0 mL of this solution was mixed with 30.0 mL of a 0.10 mol dm-³ hydrochloric acid solution. b) Using an ICE table or another appropriate method, determine the pH of the resulting buffer solution. You should show all steps in your answer.
A solution of methylamine, CH3NH2, behaves as a weak base. The equilibrium can be written as: CH3NH₂ + H+ = [CH3NH3]+ Methylamine has Kb = = 4.6 x 10-4. a) Calculate the pH of a methylamine solution with a concentration of 0.25 mol dm-³. 60.0 mL of this solution was mixed with 30.0 mL of a 0.10 mol dm-³ hydrochloric acid solution. b) Using an ICE table or another appropriate method, determine the pH of the resulting buffer solution. You should show all steps in your answer.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter14: Acids And Bases
Section: Chapter Questions
Problem 13ALQ: You mix a solution of a strong acid with a pH = 4.0 and an equal volume of another strong acid...
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A solution of methylamine, CH3NH₂, behaves as a weak base. The equilibrium can be written as:
CH3NH₂ + H+ = [CH3NH3]+
Methylamine has K₁ = 4.6 x 10-4.
a) Calculate the pH of a methylamine solution with a concentration of 0.25 mol dm-³.
60.0 mL of this solution was mixed with 30.0 mL of a 0.10 mol dm-3 hydrochloric acid solution.
b) Using an ICE table or another appropriate method, determine the pH of the resulting buffer
solution. You should show all steps in your answer.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8e2a1df8-a0ed-4597-a1d2-983ee883ee4c%2F41a7a350-eba2-4115-8d3c-117e9d3dd202%2Fa4s5e5t_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Question 4
A solution of methylamine, CH3NH₂, behaves as a weak base. The equilibrium can be written as:
CH3NH₂ + H+ = [CH3NH3]+
Methylamine has K₁ = 4.6 x 10-4.
a) Calculate the pH of a methylamine solution with a concentration of 0.25 mol dm-³.
60.0 mL of this solution was mixed with 30.0 mL of a 0.10 mol dm-3 hydrochloric acid solution.
b) Using an ICE table or another appropriate method, determine the pH of the resulting buffer
solution. You should show all steps in your answer.
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