What's the difference between an Arrhenius acid and a Bronsted-Lowry acid?

In summary, an Arrhenius acid is a substance that produces hydrogen ions when dissolved in water, while a Bronsted-Lowry acid is a substance that donates a proton to another substance in a chemical reaction. The strengths of Arrhenius acids and Bronsted-Lowry acids differ in how they are classified - Arrhenius acids based on their ability to dissociate in water and Bronsted-Lowry acids based on their tendency to donate protons. Examples of Arrhenius acids include hydrochloric acid and sulfuric acid, while examples of Bronsted-Lowry acids include acetic acid and citric acid. The acid-base reactions of Arrhenius acids and Bronsted-Lowry acids differ in the products they
  • #1
Joshua Mitchell
10
2
They both produce H+ right? How do I tell the difference in a reaction?
 
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  • #2
How come dissolving FeCl3 produces an acidic solution?
 
  • #3
Try this for a much longer discussion: http://www.chemguide.co.uk/physical/acidbaseeqia/theories.html

You can look at Bronstead-Lowry as an extension (or complement) to Arrhenius - it handles situations like the one Borek mentioned that Arrhenius does not explicitly cover.
 

FAQ: What's the difference between an Arrhenius acid and a Bronsted-Lowry acid?

What is the definition of an Arrhenius acid and a Bronsted-Lowry acid?

An Arrhenius acid is a substance that produces hydrogen ions (H+) when dissolved in water, while a Bronsted-Lowry acid is a substance that donates a proton (H+) to another substance in a chemical reaction.

How do the strengths of Arrhenius acids and Bronsted-Lowry acids differ?

Arrhenius acids are classified as strong or weak based on their ability to dissociate in water, while Bronsted-Lowry acids are classified as strong or weak based on their tendency to donate protons.

Can you give an example of an Arrhenius acid and a Bronsted-Lowry acid?

Some common Arrhenius acids include hydrochloric acid (HCl) and sulfuric acid (H2SO4), while examples of Bronsted-Lowry acids include acetic acid (CH3COOH) and citric acid (H3C6H5O7).

How do the acid-base reactions of Arrhenius acids and Bronsted-Lowry acids differ?

Arrhenius acids react with bases to form a salt and water, while Bronsted-Lowry acids react with bases to form a conjugate base and a protonated base.

Are there any similarities between Arrhenius acids and Bronsted-Lowry acids?

Both Arrhenius acids and Bronsted-Lowry acids are substances that can donate protons in a chemical reaction. Additionally, they both form a conjugate base when reacting with a base.

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