A 50 mL solution of perchloric acid of unknown concentration is titrated with a solution of lithium hydroxide of unknown concentration. It requires 30 mL of LiOH to neutralize the entire 50 mL. When 50 mL of is titrated with 10 mL of .1M KOH, it requires an additional 26.8 mL of LiOH to neutralize the perchloric acid.
(6) Classify each of the compounds as Arrhenius, Bronsted, and Lewis acids or bases.
An Arrhenius acid donates a hydrogen ion; an Arrhenius base donates a hydroxide ion. Perchloric acid donates a hydrogen and is an Arrhenius acid. The two hydroxides are Arrhenius bases. Perchloric acid donates a proton and is therefore a Bronsted acid. Since Bronsted acids are Lewis acids, is a Lewis acid. LiOH and KOH ionize in solution. The hydroxide ion acts as a proton acceptor. These two compounds are therefore Bronsted bases and hence Lewis bases.
