Lecture notes for Nov 26 Chem135 Johnson

Lecture notes for Nov 26 Chem135 Johnson - Lecture notes...

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Lecture notes for Monday, Nov 26 for Exam V Dr. Johnson CHEM135 Acid-Base Equilibrium Review LeChatelier 2NO 2  N 2 O 4 exothermic reaction ∆H negative value NO 2 brown gas Cool down on ice Temp decreased; heat removed Equilibrium shifts right to compensate Mixture of gases lighter brown Increase pressure shift to fewer moles of gas Therefore this equilibrium shifts right (in the forward direction as written above) Decrease pressure shift to more moles of gas Ther fore here shift to reactants; left; reverse B&H Chapter 11.6 Solubility Most of the chapter not covered Just know what a solubility constant is and what is represents: Solubility Product constant, K sp , is the equilibrium constant for the dissolution of an ionic solid. Example: Ca 3 (PO 4 ) 2 (s)  3 Ca 3+ (aq) + 2 PO 4 3- (aq) K sp = [Ca 2+ ] 3 [PO 4 3- ] 2- = 2.0x10 -33 Ca 3 (PO 4 ) 2 not very soluble B&H Chapter 11.7 Acids and Bases Arrhenius definition Acid is a H + donor Base is an OH - dnor Bronsted-Lowry definition Acid is a H + donor Base is a H + acceptor
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This note was uploaded on 04/07/2008 for the course CHEM 135 taught by Professor Brooks during the Fall '08 term at Maryland.

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Lecture notes for Nov 26 Chem135 Johnson - Lecture notes...

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