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Acid-Base Theories Section 20.3

Acid-Base Theories Section 20.3. Arrhenius acids : hydrogen-containing compounds that ionize to yield H + in aqueous solution. HCl + H 2 O --> H 3 O + + Cl - Arrhenius bases: compounds that ionize to yield OH - in aqueous solution 2Na + 2H 2 O --> NaOH + H 2. A few terms….

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Acid-Base Theories Section 20.3

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  1. Acid-Base TheoriesSection 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

  2. 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

  3. 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

  4. 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)

  5. 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

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