Acid-Base Theories Section 20.3

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Presentation transcript:

Acid-Base Theories Section 20.3 Arrhenius acids: hydrogen-containing compounds that ionize to yield H+ in aqueous solution. HCl + H2O --> H3O+ + Cl- Arrhenius bases: compounds that ionize to yield OH- in aqueous solution 2Na + 2H2O --> NaOH + H2

A few terms… Monoprotic acids: contain 1 ionizable hydrogen Nitric Acid HNO3 Diprotic acids: contain 2 ionizable hydrogens Sulfuric Acid H2SO4 Triprotic acids: contain 3 ionizable hydrogens Phosphoric Acid H3PO4

Bronsted-Lowry Acids and Bases Acid: hydrogen-ion donor Base: hydrogen-ion acceptor NH3 + H2O <--> NH4+ + OH- Hydrogen-ion Hydrogen-ion Ammonium ion acceptor donor

Conjugate Acid & Base Conjugate Acid: particle formed when a base gains a hydrogen ion Conjugate Base: particle that remains when an acid has donated a hydrogen ion NH3 + H2O <--> NH4+ + OH- Base Acid Conjugate Conjugate Acid Base Amphoteric: substance that acts as both an acid & a base Examples: H2O, HSO4- (Hydrogen Sulfate Ion)

Lewis Acid & Base Lewis Acid: substance that can accept a pair of electrons to form a covalent bond. Lewis Base: substance that can donate a pair of electrons to form a covalent bond. H+ + OH- --> H2O Lewis Lewis Acid Base