Let's call (C2H5)2NH simply BH.
...........BH + HOH ==> BH2 + OH^-
I..........0.133..................0...........0
C.........-x.........................x...........x
E.....0.133-x.....................x...........x
Plug the E line into the Kb expression and solve for x = (OH^-). Convert to pH. Post your work if you get stuck.
By the way, between last night and today I've worked oodles of problems for you and sarah (aka jhope). That is enough freebies. You need to show some work and thinking on your part. This is a homework help site and it's time I started HELPING and not DOING it all.
Diethylamine, (C2H5)2NH, is a weak base with Kb = 6.92×10−4 at 25 oC.
For a 0.133 mol L−1 solution of (C2H5)2NH at 25 oC, what is the percent ionization of (C2H5)2NH?
1 answer
1 answer