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# ws7302key - Worksheet 7More Solubility Problems Answer Key...

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Worksheet 7—More Solubility Problems Answer Key 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 sp = [Ag + ][Cl - ] = (9.11 x 10 -9 )(.01) = 9.11 x 10 -11 Q sp < K sp so no AgCl will precipitate [Ag + ] 9.11 x 10 -9 M [I - ] 9.11 x 10 -9 M [Cl - ] 0.01 M Are there any solid precipitates? If so how many grams of each.

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