Brønsted–Lowry theory
The Brønsted–Lowry theory, introduced in 1923, defines acids and bases based on their ability to transfer protons (H⁺ ions).
This framework expanded earlier definitions and applies to a wide variety of chemical reactions, even beyond water-based systems.
Brønsted–Lowry acid
A Brønsted–Lowry acid is a proton (H⁺) donor, which gives up a hydrogen ion in a reaction.
Brønsted–Lowry base
A Brønsted–Lowry base is a proton (H⁺) acceptor, which gains a hydrogen ion in a reaction.
Consider the reaction between hydrogen chloride (HCl) and ammonia (NH₃):
$$
\text{HCl} + \text{NH}_3 \rightarrow \text{NH}_4^+ + \text{Cl}^-
$$
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