Bronsted-Lowry definition of acid/bases
Pertaining to the Bronsted Lowry definition of acids and bases,
how come the strength of a conjugate acid or base is inversely
proprtional to the strength of the other acid/base?
It seems that the more willing a acid or base is to give up/accept
a proton, the more willing its conjugate should accept/let go of one.
Think of it this way: If strong and weak are competing, the strong one
will always win. A strong conjugate base will always attract a proton.
A strong conjugate acid will always leave its weak base. There's nothing
the weak species can do about it. Cl- is a weak base. It can't hold onto
it's proton so HCl will always completely dissociate. CH3COO- (acetate
ion) is a strong conjugate base. It doesn't want to give up the proton
and the proton can't do anything about it. So acetic acid doesn't totally
dissociate. Any clearer?
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Update: June 2012