Post a New Question

chemistry

posted by .

I need help setting up a problem to calculate pH during the titration of 20.00ml Of 0.1000M (CH3CH2)3N (Kb= 5.2 x 10-4) with 10.00ml of .1000M HCL. I can do it with a weak acid - strong base but this is a weak base - strong acid and I don't know if its the same.

It's the same process.
(C2H5)3N + HCl ==> (C2H5)3NH^+ + Cl^-

Use the Henderson-Hasslebalch equation.
I found pH = 10.72 but check that for yourself.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

More Related Questions

Post a New Question