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

Name: Problem 4, Chapter 16: Química. La ciencia central
Uploaded: 2021-08-07T11:24:09-08:00
Duration: 3 min 59 s
Channel: Sima Sarker
Description: (a) Para las bases, ¿cuál es la diferencia entre las definiciones de Arrhenius y de Brensted-Lowry? (b) Cuando el amoniaco se disuelve en agua, se comporta como una base de Arrhenius y también como una base de BronstedLowry. Explique este hecho.

(a) Para las bases, ¿cuál es la diferencia entre las definiciones de Arrhenius y de Brensted-Lowry? (b) Cuando el amoniaco se disuelve en agua, se comporta como una base de Arrhenius y también como una base de BronstedLowry. Explique este hecho.

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Key Concepts

Ammonia’s Dual Behavior in Water

When ammonia is dissolved in water, it behaves as a base under both definitions. In the Arrhenius sense, ammonia increases the concentration of hydroxide ions indirectly by reacting with water, while in the Bronsted-Lowry sense, ammonia directly accepts a proton from water. This dual behavior illustrates how ammonia fits into the broader Bronsted-Lowry framework while still meeting the criteria of the Arrhenius definition in aqueous environments.

Arrhenius Base Definition

The Arrhenius definition classifies bases as substances that increase the concentration of hydroxide ions (OH–) when dissolved in water. This definition is limited to aqueous solutions and focuses solely on the formation of OH– ions as the criterion for basicity.

Bronsted-Lowry Base Definition

The Bronsted-Lowry definition defines bases as proton (H+) acceptors. This concept is broader than the Arrhenius definition because it applies to reactions in any medium, not just aqueous solutions, and focuses on the transfer of protons rather than the formation of hydroxide ions.

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