How do you calculate the pH at the equivalence point for the titration of .190M methylamine with .190M HCl? The Kb of methylamine is 5.0 x 10-4.
We’re being asked to calculate the pH of a solution at equivalence point for the titration of 0.190 M methylamine with 0.190 M HCl.
HCl (strong acid) will react with CH3NH2 (base).
• CH3NH2 is a base and based on Bronsted-Lowry definition it is a proton acceptor.
• HCl is an acid and based on Bronsted-Lowry definition it is a proton donor.
CH3NH2(aq) + HCl(aq) ⇌ CH3NH3+(aq) + Cl-(aq)
We will calculate the pH of the solution using the following steps: