Question

How is the Bronsted-Lowry definition of an acid different from the Arrhenius definition?

• A. The Arrhenius definition says that all acids must be in aqueous solution. The Bronsted-Lowry definition says that an acid is anything that can donate a proton.
• B. The Arrhenius definition says that an acid is anything that can donate a proton. The Bronsted-Lowry definition says that all acids must be in aqueous solution.
• C. The Arrhenius definition says that anything that donates a pair of electrons is an acid. The Bronsted-Lowry definition says that an acid is anything that can donate a proton.
• D. The Arrhenius definition says that anything that donates a pair of electrons is an acid. The Bronsted-Lowry definition says that all acids must be in aqueous solution.
• E. The Arrhenius definition says that all acids must be in aqueous solution. The Bronsted-Lowry definition says that anything that can donate a pair of electrons is an acid.

Answer 1

The correct option is A The Arrhenius definition says that all acids must be in aqueous solution. The Bronsted-Lowry definition says that an acid is anything that can donate a proton.

The Arrhenius definition says that all acids must be in aqueous solution. The Bronsted-Lowry definition says that an acid is anything that can donate a proton.
An Arrhenius acid is a substance that contains hydrogen and produces hydrogen ions in solution.

$HCl\to H^{+}+C{l}^{-}$
According to Bronsted and Lowry, an acid is a proton donor.
$HCl+N{H}_3\to N{H}_4^{+}+C{l}^{-}$