posted by Nancy on .
What is the pH of a .10M (CH3)3N solution? Kb=6.40e-5
(CH3)3N + HOH ==> (CH3)3NH^+ + OH
Kb = [(CH3)3NH^+](OH^-)[CH3)3N]
Set up ICE chart, substitute into Kb expression above and solve for OH, convert to pH. Post your work if you get stuck.
I did my ice chart and found x=.00253
then i did the -log(.00253) to find the pH to be 2.597, but that's the wrong answer