In class notes for December 10, 2007

In class notes for December 10, 2007 - General Chemistry...

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General Chemistry Lecture 102a December 10, 2007 We will not cover 9-6 Final Dec 20 th 7-9pm Last lecture o Solubility o Q and Ksp Today o Separation of ions o pH dependence of solubility BaSO 4 Ksp= 1.1x10 -10 s=1.04x10 -5 Ba SO 4 Ba 2+ + SO 4 2- 0 0.10 +s +s Ksp = [BaSO 4 ][SO 4 2- ] s<<0.10 Approximately s(.10) 1.1x10 -10 = .10s S=1.1x10 -9 When you have the common ion, you always decrease the solubility. Mix 50mL, 5.0 x10 -3 M AgNO 3 with 50mL 0.250 M NaCl what are the concentrations of [Ag + ] and [Cl - ] when equilibrium is reached? Calculate Q o Q=[Ag + ][Cl - ] Ksp= 1.8 x10 -10 o [Ag + ]=50mL x (5 x 10 -3 ) = 2.5 x 10 -3 = o 100 mL o [Cl - ]= 50mL x (0.250 M) = 0.125 M o 100 mL o Q= 3.75 x 10 -4 o Q>K so precipitate should form Assume max amount of AgCl(s) forms
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General Chemistry Lecture 102a December 10, 2007 2.5 x 10 -3 mmol/mL x 100 mL = 0.250 mmol Ag + 0.125 mmol/mL x 100 mL = 12.5 mmol Cl - Ag + is the limiting reactant
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This note was uploaded on 02/22/2009 for the course CHEM 102a taught by Professor Hanusa during the Fall '06 term at Vanderbilt.

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In class notes for December 10, 2007 - General Chemistry...

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