28) Define all three definitions of acids and bases giving examples of each.
Arrhenius
Acid - Contains at least one H+ ion that when diluted, will release into water. (i.e. HNO3, H2SO4)
Base - Contains at least one OH- ion that when diluted, will release into water. (i.e. KOH, Ca(OH)2)
Bronsted-Lowry
Acid - When in a reaction, will act as a H+ ion donner, ending up as the conjugate base. (i.e. HCl, H20)
Base - When in a reaction, will act as a H+ ion acceptor, resulting as the conjugate acid. (i.e. NH3, H20)
Lewis
Acid - This type of acid must act as a electron pair acceptor in a reaction. (i.e. H+, BF3)
Base - This type of base must act as a electron pair donner in a reaction. (i.e. NH3, OH-)
