According to the Bronsted-Lowry definition, what is a base?

In the context of the Bronsted-Lowry definition, a base is specifically defined as a proton acceptor. This means that a base is capable of receiving protons (H⁺ ions) from acids during a chemical reaction. When a base accepts a proton, it typically transforms into its conjugate acid, illustrating the dynamic nature of acid-base chemistry.

The accuracy of this definition can be seen in various chemical reactions. For example, when ammonia (NH₃) reacts with water (H₂O), ammonia acts as a base by accepting a proton from water, thus forming an ammonium ion (NH₄⁺) and hydroxide ion (OH⁻). This illustrates the fundamental concept that bases increase the proton concentration in a solution by accepting protons from acids.

Understanding this definition is crucial for interpreting chemical behaviors and reactions, especially in reactions involving weak acids and bases where proton transfers are central.

This definition does not tie the concept of a base specifically to the production of hydroxide ions or electron acceptance, which are associated with different chemical definitions and contexts, such as Arrhenius bases or Lewis bases, respectively. Furthermore, while hydroxide ions are indeed related to basicity, the Bronsted-Lowry definition is