Answer:
A. Provides H in water - Arrhenius acid
B. Provides OH - in water - Arrhenius base
C. Proton donor - Bronsted-Lowry acid
D. Proton acceptor - Bronsted-Lowry base
E. Electron pair donor - Lewis base
F. Electron pair acceptor - Lewis acid.
Explanation:
Definition:
A Lewis base is any substance, such as the OH- ion, that can donate a pair of nonbonding electrons. A Lewis base is therefore an electron-pair donor.
A Bronsted-Lowry acid is a chemical species that donates one or more hydrogen ions in a reaction. Also, a Bronsted-Lowry base accepts hydrogen ions.
An Arrhenius acid is a substance that dissociates in water to form hydrogen ions or protons. In other words, it increases the number of H+ ions in the water. Also, an Arrhenius base dissociates in water to form hydroxide ions, OH-.
