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Chapter 15: Problem 3

How does Bronsted and Lowry's definition of an acid differ from Arrhenius's definition of an acid? Explain which definition is broader.

Short Answer

Expert verified
According to Bronsted-Lowry, an acid is a proton donor, while Arrhenius describes an acid as a substance that increases the concentration of H+ ions when dissolved in water. The Bronsted-Lowry definition is broader as it includes every molecule or ion capable of donating a proton, regardless of the presence of water.

Step by step solution

01

Definition of an Acid According to Bronsted-Lowry

Bronsted and Lowry defined an acid as a proton donor, that is, any substance that can donate a hydrogen ion H+ is considered an acid.
02

Definition of an Acid According to Arrhenius

Arrhenius defined an acid as a substance that increases the concentration of H+ ions when dissolved in water. This means that an acid, according to Arrhenius, is a substance that when in aqueous solution will ionize or dissociate to produce H+ ions or protons.
03

Determining Which Definition is Broader

Comparing the two definitions, the Bronsted-Lowry definition is broader than the Arrhenius definition. This is because, according to Bronsted-Lowry, every molecule or ion capable of donating a proton is considered an acid, even if the process does not occur in water. Therefore, this definition includes more chemical species as acids.

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Most popular questions from this chapter

To standardize a hydrochloric acid solution, it was used as titrant with a solid sample of sodium hydrogen carbonate, NaHCO \(_{3} .\) The sample had a mass of \(0.3967 \mathrm{g},\) and 41.77 \(\mathrm{mL}\) of acid was required to reach the equivalence point. Calculate the concentration of the standard solution.

Describe two precautions that should be taken to ensure an accurate titration.

Calculate the \(\mathrm{pH}\) of a 0.0316 \(\mathrm{M}\) solution of the strong base RbOH.

What product do all neutralization reactions have in common?

Find the \(\mathrm{pH}\) of a solution consisting of 0.29 mol of \(\mathrm{HBr}\) in 1.0 \(\mathrm{L}\) of water.
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