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H2SO4.... and Lewis Bases?
Can Sulfuric Acid be a Lewis Base? It has nonbonding pairs of electrons, so can it donate any?
3 Answers
- pisgahchemistLv 79 years agoFavorite Answer
H2SO4 is not a Lewis base in aqueous solution. It doesn't exist as the molecule in aqueous solution. In aqueous solution it dissociates completely to form H+ and HSO4^- since it is a strong acid. A Lewis base is an electron pair donor. HSO4- could react with Ba2+ to form BaSO4 and H+ in which case SO4^3- would be a Lewis base.
But in "pure" sulfuric acid, aka concentrated sulfuric acid, H2SO4 can undergo autoionization to make HSO4- and H3SO4^+. In that case H2SO4 is amphoteric and acts as both an acid and a base.
============ Follow up ============
Linda said, "H2SO4 is a Lewis acid because it acts as a source of H+." No. That makes H2SO4 a Bronsted-Lowry acid, not a Lewis acid. A Lewis acid is defined an an electron pair acceptor. A Bronsted-Lowry acid is a "proton" donor. (H+ is a proton.)
- 9 years ago
Sulfuric Acid is a Lewis Acid since it ACCEPTS a pair of electrons from a Lewis Base, it does not donate electrons.
H2SO4 is a Lewis acid because it acts as a source of H+.
When a Lewis base removes the proton from H2SO4, the O—H bond is broken and the electrons in the bond become localized on the oxygen and then have resonance with the other lone pair electrons on oxygen in the sulfate ion, HSO4-.
