11.4 - Chem 102B Discussion Worksheet #18 The Brnsted-Lowry...

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Chem 102B – Discussion Worksheet #18 The Brønsted-Lowry definition of an acid is a substance capable of donating a proton (H + ), and a base is a substance capable of accepting a proton . For example, the weak acid, HF , can be dissolved in water, giving the reaction: In this reaction, HF is the species losing a proton (H + ), thus making HF an acid . Water is the species accepting the proton, to form the hydronium ion, H 3 O + , making it the base . F - (aq) is the conjugate base of HF. It can act as a base by gaining a proton in the reverse reaction. H 3 O + is the conjugate acid of H 2 O, since it can lose a proton in the reverse reaction. The stronger an acid the weaker its conjugate base; the stronger the base, the weaker its conjugate acid. The equilibrium concentrations of these species will be determined by the relative strengths of the acids and bases. The strongest acid will dissociate to the greatest extent. The equilibrium state is described by an equilibrium constant K a
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This note was uploaded on 02/14/2011 for the course CHEMISTRY 102 taught by Professor Whitt during the Spring '11 term at University of Illinois, Urbana Champaign.

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11.4 - Chem 102B Discussion Worksheet #18 The Brnsted-Lowry...

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