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Consider a solution that is 1.3×10−2 M in Ba2+ and 1.8×10−2 M in Ca2+. Ksp(BaSO4)=1.07×10−10 Ksp(CaSO4)=7.10×10−5...

Consider a solution that is 1.3×10−2 M in Ba2+ and 1.8×10−2 M in Ca2+. Ksp(BaSO4)=1.07×10−10 Ksp(CaSO4)=7.10×10−5

*Part A: If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first?

A) Ba2+ (ANSWER)

B) Ca2+

*Part B: What minimum concentration of Na2SO4 is required to cause the precipitation of the cation that precipitates first? Express your answer using two significant figures.

[Na2SO4][ N a 2 S O 4 ] = 8.2×10−9 M (ANSWER)

*Part C: What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate? Express your answer using two significant figures.

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Basla = Bulbst Schcom) Carson 3 Ca2() + SC27 (22) Some Beluet & Clancy - (Bast] * [sch] Q Care = [Czt] * [SCP] When a holoks

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Consider a solution that is 1.3×10−2 M in Ba2+ and 1.8×10−2 M in Ca2+. Ksp(BaSO4)=1.07×10−10 Ksp(CaSO4)=7.10×10−5...
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