What does Brønsted-Lowry acid-base theory state?

The Brønsted-Lowry acid-base theory provides a fundamental understanding of acid-base reactions by focusing on the transfer of protons (H⁺ ions). According to this theory, an acid is defined as a substance that donates a proton, while a base is defined as a substance that accepts a proton. This definition expands the concept of acids and bases beyond just those substances that produce hydrogen ions (H⁺) or hydroxide ions (OH⁻) in water, as seen in Arrhenius theory.

This viewpoint is crucial because it allows for the identification of acids and bases in a wider range of reactions, including those that do not occur in an aqueous environment. For example, ammonia (NH₃) can act as a base by accepting a proton from a more acidic substance, even though it doesn’t produce hydroxide ions.

In contrast, other choices misrepresent the relationships defined by the Brønsted-Lowry theory. The notion that an acid accepts a proton or that all bases are classified as proton donors diverges from the key principles of this acid-base definition. Furthermore, stating that the theory does not categorize acids or bases contradicts its very purpose, which is to classify substances based on their ability to