Final answer:
The main difference between Arrhenius and Brønsted-Lowry acids is that Arrhenius acids produce hydrogen ions in aqueous solutions, whereas Brønsted-Lowry acids are proton donors regardless of the solution. Arrhenius bases produce hydroxide ions in solution, while Brønsted-Lowry bases accept protons.
Step-by-step explanation:
Arrhenius vs. Brønsted-Lowry Acids
The distinction between Arrhenius acids and Brønsted-Lowry acids lies in their definitions and the scope of chemical species they include. An Arrhenius acid is a substance that produces hydrogen ions (H+) in aqueous solution, indicating its propensity to increase the concentration of H+ when dissolved in water. In contrast, a Brønsted-Lowry acid is broadly defined as a proton donor, which means any species that donates a hydrogen ion in a chemical reaction, not just in aqueous solution. Similarly, an Arrhenius base produces hydroxide ions (OH−) in solution, while a Brønsted-Lowry base is a proton acceptor, which can be any species that accepts a hydrogen ion in a chemical reaction.
For example, hydrochloric acid (HCl) is an Arrhenius acid as it produces hydrogen ions in water (HCl → H+ + Cl−), and it is also a Brønsted-Lowry acid because it donates a proton to another species. On the other hand, ammonia (NH3) doesn't produce hydrogen ions in aqueous solution but can accept a proton to form NH4+, thereby acting as a Brønsted-Lowry base, but not an Arrhenius base.