What is a Bronsted-Lowry base?

A Bronsted-Lowry base is defined as a substance that accepts a proton (H⁺ ion) from another substance during a chemical reaction. This concept was introduced by the Bronsted-Lowry theory, which focuses on the transfer of protons in acid-base reactions.

When a base accepts a proton, it becomes its conjugate acid, showcasing the dynamic nature of acid-base chemistry as reactions can shift depending on the nature of the reactants involved. For example, if ammonia (NH₃) acts as a Bronsted-Lowry base by accepting a proton, it forms ammonium (NH₄⁺), demonstrating how substances can act differently based on the environmental context of the reaction.

This understanding is crucial in predicting the behavior of various substances in chemical reactions, especially in biological and aqueous environments where proton transfer is fundamental. Hence, any substance that can accept a proton qualifies as a Bronsted-Lowry base, which is also key in understanding the underlying mechanisms of buffers, equilibrium, and reaction pathways in chemistry.