[XxslbabesxX]

Is it possible for someone to give me an example of a Bronstead-Lowry acid that isn't a Arrehenius acid? I'm studying the two now and I think it might be helpful if I can see the difference. Thank you in advance.

[Borek]

a bronsted acid is a proton donor
an arrhenius acid is a H+ donor

What is a difference between H+ and proton?

[Borek]

Are you sure the Arrhenius definition mention 'donors'? IIRC it speaks only about dissociation...

[Dude]

My take is that all Arrhenius acids are Bronsted-Lowry acids and there are no examples of an acid in one model that isn't in the other model.  The difference between the two models is in the base.  Arrhenius strictly defined a base as a hydroxide, whereas the Bronsted-Lowry model broadened the definition of a base to a proton acceptor.  Therefore,
HCl + NaOH -->  NaCl + H2O  Arrhenius + Bronsted-Lowry acid/base
HCl + H2O ----> H30+  + Cl-   Bronsted/Lowry acid/base   Arrhenius - H2O is not a base since it does not contain OH- equation not defined by Arrhenius model