At what molarity will 0.100 M Ca2+ begin to precipitate out of a solution of KAl(SO4)2?(Ksp of CaSO4=2.4x10-5) 2.4x10-4M KAl(SO4)2 4.9x10-3M KAl(SO4)2 2.4x10-3M KAl(SO4)2 1.2x10-4 M KAl(SO4)2
At what molarity will 0.100 M Ca2+ begin to precipitate out of a solution of KAl(SO4)2?(Ksp of CaSO4=2.4x10-5) 2.4x10-4M KAl(SO4)2 4.9x10-3M KAl(SO4)2 2.4x10-3M KAl(SO4)2 1.2x10-4 M KAl(SO4)2
Chemistry by OpenStax (2015-05-04)
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Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
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Chapter15: Equilibria Of Other Reaction Classes
Section: Chapter Questions
Problem 40E: A volume of 0.800 L of a 2104 -M Ba(NO3)2 solution is added to 0.200 L of 5104M Li2SO4. Does BaSO4...
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At what molarity will 0.100 M Ca2+ begin to precipitate out of a solution of KAl(SO4)2?(Ksp of CaSO4=2.4x10-5)
2.4x10-4M KAl(SO4)2 | |
4.9x10-3M KAl(SO4)2 | |
2.4x10-3M KAl(SO4)2 | |
1.2x10-4 M KAl(SO4)2 |
Expert Solution
Step 1
Given : Concentration of Ca2+ ions = 0.100 M
And Ksp of CaSO4 = 2.4 X 10-5
The solubility reaction of CaSO4 can be written as,
=> CaSO4 (s) --------> Ca2+ (aq) + SO42- (aq) Ksp = 2.4 X 10-5
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