Chem2 - Unit P Acid Base (Proton) Reactions Acid bases have...

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Acid Base (Proton) Reactions Acid bases have to work in water – solution Acids donate H + Base donate OH - P.2 Bronsted-Lowry Theory of Acids and Bases An acid base reaction is a proton-transfer reaction in which the proton is transferred from the acid to the base. An acid is a proton donor, and a base is a proton acceptor (according to this theory, anything that can receive a proton is a base) (base should be negatively charged) - acid proton donor, H + - base proton acceptor .. - always have acid-base pairs; H – O – H + NH 3 H – O : - + NH 4 + (acid) (base) (base) . . (acid) (gave up a proton) (acceptor) the stronger the acid, the weaker its conjugate base, see table P.1 ex: perchloric acid (strong acid) (H3O+) (weak base) HClO 4 H + + ClO 4 - equilibrium HClO 4 H + + ClO 4 - Equilibrium is going to favor the weak acid P.8 Water Equilibrium HOH H + (aq) + OH - (aq) kw = equilibrium constant for H 2 O kw = [H + ][OH - ] = [H + ][OH - ] = 1.0 x 10
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This note was uploaded on 09/02/2011 for the course CHEM 2 taught by Professor Harrison during the Spring '11 term at West Valley.

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Chem2 - Unit P Acid Base (Proton) Reactions Acid bases have...

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