- #1
Joshua Mitchell
- 10
- 2
They both produce H+ right? How do I tell the difference in a reaction?
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.
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.
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).
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.
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.