Which statement correctly defines a conjugate base?

A conjugate base is defined as the species that remains after an acid has donated a proton (H+ ion) during a chemical reaction. This process is part of the Bronsted-Lowry theory of acids and bases, which characterizes acids as proton donors and bases as proton acceptors. When an acid releases a proton, it transforms into its corresponding conjugate base.

For example, if we take acetic acid (CH3COOH) as our acid, when it donates a proton, it becomes the acetate ion (CH3COO−), which is the conjugate base. Therefore, the definition of a conjugate base aligns perfectly with the statement that it results when an acid donates a proton.

Understanding this concept is crucial when analyzing acid-base reactions, as it helps identify the relationship between acids and their conjugate bases, further illustrating their role in equilibrium dynamics within chemical reactions.