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:
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.
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Weak Base Strong Acid Titrations concept. You can view video lessons to learn Weak Base Strong Acid Titrations. Or if you need more Weak Base Strong Acid Titrations practice, you can also practice Weak Base Strong Acid Titrations practice problems.