chapter4 - CHM 291 9-24 CHP 4 Problems 4.1-26, 29-38, 40,...

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CHP 4 Problems 4.1-26, 29-38, 40, 42, 45. 4.0 The Acid-Base Reaction The acid-base reaction is a chemical reaction involving the transfer of an electron. These reactions are typically equilibria. 4.1 Definitions Bronsted-Lowry – Acid is a proton donor. Base is a proton acceptor. B: + H - A + B - H + :A - In the reverse reaction + B - H is the conjugate acid and :A - is the conjugate base. Figure 4.1 Lewis – Acid is an electron pair acceptor. Base is an electron pair donor. Example: 4.2 The Acid Base Equilibrium The equilibrium constant for the reaction of many acids with water (base) have been determined and termed acid dissociation constants. The equilibrium constant for this reactions is: Since water is the solvent and in large excess. The concentration is constant. This allows the use of the acidity constant ( K a ). Due to the large range of acidity constants a logarithmic scale is usually used. p K a = -log K a Smaller p K a (larger K a ) is a stronger acid. Base strengths can be determined from the p
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This note was uploaded on 04/17/2009 for the course CHM 227 taught by Professor Rosen during the Fall '08 term at Rhode Island.

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chapter4 - CHM 291 9-24 CHP 4 Problems 4.1-26, 29-38, 40,...

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