Superbase - Simple English Wikipedia, the free encyclopedia

Acids and bases
Acceptor number Acid Acid–base reaction Acid–base homeostasis Acid strength Acidity function Amphoterism Base Buffer solutions Dissociation constant Donor number Equilibrium chemistry Extraction Hammett acidity function pH Proton affinity Self-ionization of water Titration Lewis acid catalysis Frustrated Lewis pair Chiral Lewis acid
Acid types
Brønsted–Lowry Lewis Mineral Organic Oxide Strong Superacids Weak Solid
Base types
Brønsted–Lowry Lewis Organic Oxide Strong Superbases Non-nucleophilic Weak

In chemistry, a superbase is an extremely strong base. It is a compound that has a high affinity for protons.

Hydroxide ion is the strongest base possible in water (aqueous) solutions, but superbases are much stronger than aqueous bases. Such bases are useful in organic synthesis and are fundamental to physical organic chemistry.

Superbases have been described and used since the 1850s.^[1] Reactions involving superbases often require special techniques since they are destroyed by water, carbon dioxide, and oxygen in the air. Inert atmosphere techniques and low temperatures minimize these side reactions.

IUPAC defines superbases simply as a "compound having a very high basicity, such as lithium diisopropylamide".^[2]

• Superacid

1. ↑ "BBC - h2g2 - History of chemistry - acids and bases". Retrieved 2009-08-30.
2. ↑ "IUPAC Gold Book - superacid". Retrieved 2009-08-30.