What is Bronsted Lowry Theory of Acids in College Chemistry?

Learn Bronsted Lowry Theory of Acids definition in college chemistry with explanation to study “What is Bronsted Lowry Theory of Acids”. Study bronsted lowry theory of acids explanation with college chemistry terms to review chemistry course for online degree programs.

Bronsted Lowry Theory of Acids Definition

Bronsted Lowry Theory of Acids Explanation

According to the bronsted- lowry theory any compound that can transfer a proton to any other compound is an acid, and the compound that accepts the proton is a base. To denote proton we also use H+ as it constitutes the nucleus of a hydrogen atom. The major concept of this theory is that a substance can function as an acid only in the presence of a base and similarly a substance can function as a base only in the presence of an acid. A common example is the reaction between an acidic substance, such as hydrochloric acid, and a basic substance, such as ammonia. As a result we obtain an ammonium ion and a chloride ion. The ammonium ion is the acid conjugate to the base ammonia while the chloride ion is the base conjugate to the hydrochloric acid. This theory has great significance in chemistry.

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