In the context of the Bronsted-Lowry theory, what defines bases?

In the Bronsted-Lowry theory, bases are defined as substances that accept protons (H⁺ ions). This theory expands the traditional definition of acids and bases, focusing on proton transfer during chemical reactions. When a base accepts a proton, it can often form a conjugate acid, demonstrating its ability to interact with protons in a chemical reaction.

The key component of this definition is the focus on proton acceptance, distinguishing bases from acids, which are characterized as proton donors. Unlike other concepts in chemistry, such as the Lewis theory — which emphasizes electron pair acceptance — the Bronsted-Lowry framework provides a clear mechanism of acid-base interactions based on protons.

The other options do not accurately align with the Bronsted-Lowry definition. While substances forming salts or increasing acidity may relate to acid-base reactions, they do not specifically capture the fundamental role of bases as proton acceptors. Thus, the distinction is crucial in understanding the dynamic nature of acid-base chemistry as described by the Bronsted-Lowry theory.