Example of a substance that is a Bronsted-Lowry, but not Arrhenius

pinkyjoshi65

Could someone give and example of a substance that is a Bronsted-Lowry base, but not an Arrhenius base..

staf9

Ammonia (NH3)

Accepts a proton (Bronsted-Lowry), yet does not disassociate hydroxide ions into water (not Arrhenius)

astro_kat

no think about Lewis acids/bases

staf9

Lewis bases are defined as being able to donate a pair of electrons, ammonia also falls into this category... is that what you mean?

NH3 is generally regarded as not an Arrhenius base since it autoionizes and is amphoteric:

NH3 + NH3 ⇄ NH4+ + NH2-