Which statement best describes a Bronsted-Lowry base?

A Bronsted-Lowry base is defined as a substance that accepts protons (H⁺ ions) during a chemical reaction. This theory, formulated by Johannes Bronsted and Thomas Lowry, focuses on the transfer of protons between substances. According to this definition, when a base encounters an acid (which is a substance that donates protons), the base accepts the proton from the acid, forming a conjugate acid in the process.

This concept is fundamental in understanding acid-base reactions because it shifts the focus from the traditional Lewis acid-base theory, which defines acids and bases in terms of electron pair donors and acceptors. In many reactions, especially in many biological processes, the transfer of protons is more significant, making the Bronsted-Lowry definition particularly useful.

While other options describe different properties or characteristics of substances, they do not align with the specific function of a Bronsted-Lowry base. For example, donating electrons refers to leptonic behavior, which pertains to Lewis bases, and dissociating in water or having a negative charge does not necessarily dictate a substance's ability to accept protons. Thus, the accurate representation of a Bronsted-Lowry base is indeed that it accepts protons.