ws8s08vkey - Work Sheet 8+ CH302 Spring 2008 1. A solution...

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Work Sheet 8+ CH302 Spring 2008 1. A solution is made with NaI and NaCl such that it is 0.01 M in both I - and Cl - . To 1 L of this solution 0.01 moles Ag(NO 3 ) are added (you can ignore any volume change). The NaI, NaCl, and Ag(NO 3 ) are completely soluble (as is NaNO 3 but you already knew that). The K SP for AgI is 8.3 x 10 -17 and for AgCl is 1.8 x10 -10 . After the solution has reached equilibrium what are the concentrations of the following? Will anything precipitate? Initial concentration of [Ag + ] is 0.01 M, [I - ] = 0.01 M, [Cl - ] = 0.01 M Q sp = [Ag + ][I - ] = (.01)(.01) = 10 -4 AgI could precipitate Q sp = [Ag + ][Cl - ] = (.01)(.01) = 10 -4 AgCl could precipate However AgI is much less soluble than AgCl. Assume the AgI precipitates completely to equilibrium Then you have a saturated solution of AgI Concentration of Ag + will be K sp = [Ag + ][I - ] [Ag + ] = sqrt(K sp ) = sqrt(8.3 x 10 -17 ) = 9.11 x 10 -9 Given this concentration will the AgCl precipitate? Q

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This homework help was uploaded on 04/12/2008 for the course CH 302 taught by Professor Holcombe during the Spring '07 term at University of Texas at Austin.

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ws8s08vkey - Work Sheet 8+ CH302 Spring 2008 1. A solution...

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