According to the Brønsted-Lowry theory, what are acids?

In the context of the Brønsted-Lowry theory, acids are defined as substances that donate protons (H⁺ ions) to other substances. This definition emphasizes the role of protons in chemical reactions, where the transfer of protons is a key component of acid-base interactions. When a substance donates a proton, it effectively increases the concentration of protons in the solution, thereby exhibiting acidic properties.

This understanding of acids as proton donors is foundational to predicting and explaining the behavior of various chemical substances in reactions. For instance, when hydrochloric acid (HCl) is dissolved in water, it donates a proton to water, forming hydronium ions (H₃O⁺) and chloride ions (Cl⁻).

In contrast, bases are defined by the Brønsted-Lowry theory as proton acceptors, which highlights the reciprocal nature of acid-base reactions. This view broadens the understanding of acids and bases beyond just the presence of hydroxide ions or the traditional definitions, as it allows for more complex interactions in various environments.

Recognizing acids as proton donors allows students to apply this concept across various scenarios in chemistry, aiding in understanding reaction mechanisms and the properties of various substances in