Classify the following as Arrhenius, Brønsted-Lowry, or Lewis acid-base reactions. A reaction may fit all, two, one, or none of the categories: (1) Ag + + 2NH3 LaTeX: \leftrightarrow↔Ag(NH3)2+ (2) H2SO4 + NH3 LaTeX: \leftrightarrow↔HSO42-+ NH4+ (3) 2HCl LaTeX: \leftrightarrow↔H2 + Cl2 (4) AlCl3 + Cl- LaTeX: \leftrightarrow↔AlCl4- A. Arrhenius acid-base reactions B. Brønsted-Lowry acid-base reactions C. Lewis acid-base reactions

Explanation:

An Arrhenius acid is a substance that dissociates in water to form hydrogen ions (H+). In other words, an acid increases the concentration of H+ ions in an aqueous solution.

An acid-base reaction according to the Brønsted-Lowry definition is a transfer of a proton from one molecule or ion to another. Bronsted-Lowery definition refers to the loss or gain of an H+ (proton). The acid is a proton donor, and the base is a proton acceptor.

A Lewis acid-base reaction is a chemical reaction that forms at least one covalent bond between an electron pair donor (Lewis base) and an electron pair acceptor (Lewis acid). Lewis theory of acid-base reactions, bases donate pairs of electrons and acids accept pairs of electrons.

1. Ag+ + 2NH3 ⇌ Ag(NH3)2 -

C

2. H2SO4 + NH3 ⇌ HSO4- + NH4+

A, B

3. 2HCl ⇌ H2 + Cl2

None

4. AlCl3 + Cl- ⇌ AlCl4-

C