(a) Para los ácidos, ¿cuál es la diferencia entre las...

(a) Para los ácidos, ¿cuál es la diferencia entre las definiciones de Arrhenius y de Bronsted-Lowry? (b) $\mathrm{El} \mathrm{NH}_3(\mathrm{~g})$ y el $\mathrm{HCl}(g)$ reaccionan para formar el sólido iónico $\mathrm{NH}_4 \mathrm{Cl}$ (s) (Figura 16.3). En esta reacción, ¿cuál sustancia es el ácido de Brrnsted-Lowry? ¿Cuál es la base de Bronsted-Lowry?

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Key Concepts

Arrhenius Acid Definition

The Arrhenius definition of acids is based on the idea that an acid is a substance that increases the concentration of H+ (hydrogen) ions in an aqueous solution. This definition focuses on the behavior of the substance in water, limiting its scope to reactions in an aqueous environment, and it primarily defines acids by the ions they release upon dissolution.

Bronsted-Lowry Acid-Base Theory

The Bronsted-Lowry theory broadens the concept of acids and bases by defining an acid as a proton donor and a base as a proton acceptor. This definition is not limited to aqueous solutions and focuses on the transfer of protons (H+ ions) during a reaction. It provides a more general framework for understanding acid-base reactions in a variety of chemical environments.

Identification of Acids and Bases in Reactions

In applying the Bronsted-Lowry concept to chemical reactions, one identifies the acid as the species that donates a proton, and the base as the species that accepts a proton. This approach is used to analyze reactions by tracking the movement of protons, allowing for the determination of which substances act as acids and bases even in non-aqueous or gas phase reactions.

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