Final answer:
The Arrhenius definition of acids and bases is limited to substances that dissociate to produce specific ions in water, while the Brønsted-Lowry definition is more general and includes proton transfer reactions in any solvent.
Step-by-step explanation:
The Arrhenius definition of acids and bases is somewhat limited, as it only considers substances that dissociate to produce hydronium ions (H3O+) as acids and hydroxide ions (OH-) as bases in aqueous solutions. On the other hand, a Brønsted-Lowry base is defined as a molecule or ion that accepts a hydrogen ion (proton), while a Brønsted-Lowry acid is a molecule or ion that donates a hydrogen ion in a reaction. The concept of Brønsted-Lowry acids and bases is more general than the Arrhenius definition, as it includes substances that can undergo proton transfer reactions in any solvent, not just water.