Kaplan Nursing Entrance Practice Exam

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What defines a Bronsted-Lowry base?

Species that donates protons
Species that accepts protons
Substance that remains neutral
Species that releases hydroxide ions

The correct answer is: Species that accepts protons

A Bronsted-Lowry base is defined as a species that accepts protons (H⁺ ions). This definition is part of the Bronsted-Lowry theory of acids and bases, which was established to broaden the understanding of acid-base reactions beyond just those involving hydroxide ions. In this context, a base is characterized by its ability to increase the concentration of OH⁻ in a solution by accepting protons from the surrounding environment or from acids. For instance, when ammonia (NH₃) reacts with water, it accepts a proton from the water, forming ammonium (NH₄⁺) and hydroxide (OH⁻). This ability to accept protons is fundamental to understanding acid-base chemistry, making it a key concept for nursing students to master as they consider drug interactions, physiological changes, and pH balance in the human body. Other definitions provided do not precisely align with the Bronsted-Lowry definition of a base—donating protons defines an acid, remaining neutral does not pertain to acids or bases specifically, and releasing hydroxide ions is more in line with the Arrhenius definition of a base rather than the Bronsted-Lowry framework.