Which of the following describes the strongest conjugate base paired with a Bronsted-Lowry acid?

The strongest conjugate base corresponds to the weakest Bronsted-Lowry acid. This relationship is rooted in the concept of acid-base equilibrium. According to the Bronsted-Lowry theory, an acid is a proton donor, while a base is a proton acceptor.

When an acid donates a proton, it transforms into its conjugate base. The strength of an acid is inversely related to the strength of its conjugate base; thus, the weaker the acid, the stronger its conjugate base will be. This is due to the fact that a weak acid does not dissociate completely, leaving a significant concentration of its conjugate base in solution, which can readily accept protons.

For example, consider acetic acid (a weak acid) compared to hydrochloric acid (a strong acid). The conjugate base of acetic acid is acetate, which is a relatively strong base as it can easily accept protons. In contrast, the conjugate base of hydrochloric acid is chloride, which is weak and does not readily accept protons because hydrochloric acid fully dissociates in water.

This relationship highlights the fundamental principle that the strength of a conjugate base is determined by the dissociation characteristics of its parent acid, leading to