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Chapter 4: Problem 26

Give Arrhenius's and Bronsted's definitions of an acid and a base. Why are Bronsted's definitions more useful in describing acid-base properties?

Short Answer

Expert verified
According to Arrhenius, acids increase the concentration of H+ ions in water and bases increase the concentration of OH- ions. Bronsted defines acids as proton donors and bases as proton acceptors, making his definitions more useful as they include more substances and are not restricted to aqueous solutions.

Step by step solution

01

Arrhenius's Definitions

Arrhenius's theory identifies an acid as a substance that increases the concentration of hydrogen ions (H+) when dissolved in water, and a base as a substance that increases the concentration of hydroxide ions (OH-) when dissolved in water.
02

Bronsted's Definitions

On the other hand, according to Bronsted's theory, an acid is a substance that can donate a proton (H+), and a base is a substance that can accept a proton.
03

Comparing Both Definitions

While both theories correctly identify the presence of H+ ions in acid and OH- ions in base, Bronsted's definitions are more general. They do not restrict the definition of acids and bases to aqueous solutions, and include more substances under the category of acids and bases.
04

Why Bronsted's Definitions Are More Useful

Bronsted's definitions are more useful because they include a broader range of substances as acids and bases. They also explain the acid-base behaviour of substances in non-aqueous solutions and allow us to study proton donating-accepting behaviour even for substances which do not form hydrogen or hydroxide ions in solution. They allow us to explain acid-base reactions where there is no water involved at all.

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