KI(aq) is slowly added to a solution with [Pb2+] = [Ag-] = 0.10 M Ksp values: AgI = 8.5 x 10⁻17 PbI2 = 7.1 x 10-9 1. Calculate the [I⁻] needed to precipitate AgI. 2. Calculate the [I⁻] needed to precipitate PbI2 . 3. Which precipitate should form first, AgI or PbI2 ?
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KI(aq) is slowly added to a solution with [Pb2+] = [Ag-] = 0.10 M
Ksp values: AgI = 8.5 x 10⁻17 PbI2 = 7.1 x 10-9
1. Calculate the [I⁻] needed to precipitate AgI.
2. Calculate the [I⁻] needed to precipitate PbI2 .
3. Which precipitate should form first, AgI or PbI2 ?
4. Calculate the concentration of the first cation to precipitate that remains in solution when the second cation begins to precipitate?
5. Can Ag+(aq) and Pb2+(aq) be effectively separated by fractional precipitation of their iodides? Justify your answer.
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