Strong bronsted lowry acids are H+ donors, bases are proton acceptors. Lewis acids are electron pair acceptors, and Lewis bases are electron pair donors.
Thank you soo much, that makes so much sense :)
But saying completely ionized is not necessarily correct. A strong acid such as HCl will be completely ionized in the presence of a weak or a strong base, but a strong acid like H3PO4 will give up the its first proton readily in a solution with a weak or strong base, but its conjugate acid will not readily due so with the weak base. So, saying completely ionized isn't necessarily correct, but saying readily able to give up A proton with a weak base such as H20, which can act as an acid or a base, is better. I could be wrong, but this is the way I understand it.
Thank you soo much :) I can totally see you as a smart Chemist in the future :)
I'm actually a biochemist, I just haven't been immersed in some of this stuff in a while. My last post should read conjugate base not acid. Sorry for that, I'm a little prone to typos and brain farts when I'm a little tired.
Although all of H3PO4 is completely ionized (i.e, -H2PO4,) it can not give up the rest of its H+ readily.
and when you think of strong bronsted lowry acid you think of strong proton donors.