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