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: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 32QRT

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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