What does a conjugate base correspond to in Bronsted-Lowry theory?

In Bronsted-Lowry theory, a conjugate base is defined as what remains after an acid donates a proton (H⁺). This means that when an acid loses a proton, it turns into its conjugate base. Therefore, a conjugate base corresponds to a pair with its Bronsted-Lowry acid, as they are related by the transfer of a proton.

Understanding this relationship is key in analyzing acid-base reactions, as every acid has a corresponding conjugate base. The concept emphasizes the dynamic equilibrium in acid-base chemistry, where the transfer of protons defines the behavior of these species in various reactions.

The other choices do not accurately capture the definition of a conjugate base in this context. A conjugate base does not receive a proton, as that would be representative of a conjugate acid instead. It also does not pair with a Bronsted-Lowry base; rather, it is formed from an acid. And while a conjugate base is related to an acid, it itself is not an acid, reinforcing the notion that it is specifically the species created when an acid loses a proton.