How do Bronsted-Lowry acids and bases typically differ from traditional Arrhenius definitions?

Bronsted-Lowry acids and bases provide a broader and more versatile framework for understanding acid-base chemistry compared to the traditional Arrhenius definitions. The key aspect of the Bronsted-Lowry theory is that it defines acids as proton donors and bases as proton acceptors. This definition moves beyond the limited scope of the Arrhenius theory, which strictly classifies acids as substances that increase the concentration of hydrogen ions (H⁺) in water and bases as those that increase the concentration of hydroxide ions (OH⁻) in water.

By recognizing the role of proton transfer, the Bronsted-Lowry theory allows for the classification of acid-base reactions that occur in non-aqueous solvents or even in gas-phase reactions, where the presence of water is not a factor. This makes it a more holistic approach to acid-base behavior in various chemical environments. In contrast, the Arrhenius definition is limited to aqueous solutions, which restricts its applicability in a wider range of chemical contexts. Thus, the importance of proton transfer is central in distinguishing the Bronsted-Lowry theory from the Arrhenius concept.