In the Bronsted-Lowry model of acids and bases, a(n) _ is a hydrogen donor and a(n) _ is a hydrogen acceptor. A. acid, base B. base, acid C. conjugate acid, conjugate base D. conjugate base, conjugate acid
The Correct Answer and Explanation is:
The correct answer is A. acid, base.
In the Bronsted-Lowry model, acids and bases are defined by their ability to donate or accept protons (hydrogen ions). An acid is a hydrogen donor, meaning it releases a proton (H⁺) when it reacts with a base. A base, on the other hand, is a hydrogen acceptor, meaning it accepts a proton during the reaction.
To clarify, a Bronsted-Lowry acid will lose a hydrogen ion, leaving behind its conjugate base. Conversely, a Bronsted-Lowry base will accept a proton and become a conjugate acid. For example, when hydrochloric acid (HCl) dissolves in water, it donates a proton to water, forming the hydronium ion (H₃O⁺) and the chloride ion (Cl⁻). In this case, HCl is the acid because it donates a proton, and H₂O (water) acts as the base because it accepts the proton.
The key feature of the Bronsted-Lowry model is that the role of acids and bases is not fixed and can depend on the specific reaction. For example, in a different context, water might act as an acid by donating a proton, while a substance like ammonia (NH₃) would act as a base by accepting it.
The Bronsted-Lowry model focuses more on the transfer of protons rather than the involvement of electrons, making it a broader and more versatile definition of acids and bases compared to other models, such as the Lewis model. By focusing on proton transfer, it provides a clearer understanding of many acid-base reactions, especially in aqueous environments.
