| Since there's supposed be a lot of equilibrium on the test, here's one:
Calculate the pH at the equivalence point in the titration of 50 mL of .10 M methylamine (CH3NH2) with a .20M HCl.
Kb of CH3NH2 (methylamine): 4.4*10^-4 or Ka of CH3NH3+ : 2.3*10^-11
HINT: This is a weak base, strong acid titration, so you need to eventually find the pH for the hydrolysis of CH3NH3+ with ICE charts and approximation. |