Asked by kellie
The Ksp for calcium fluoride (CaF2) is 3.9 x 10^–11 at 25°C. How many moles of solid NaF must be added to 1.00 L of 0.100 M CaCl2 in order to precipitate CaF2?
Please help me set up this ICE table and understand how to solve this!! thank you!!
Please help me set up this ICE table and understand how to solve this!! thank you!!
Answers
Answered by
DrBob222
(Ca^2+) = 0.1M
Ksp = (Ca^2+)(F^-)2
Substitute 0.1M for Ca^2+ and solve for (F^-) in mols/L.
You have 1.00 L so that is the number of mols F^- (= mols NaF) that must be added.
Ksp = (Ca^2+)(F^-)2
Substitute 0.1M for Ca^2+ and solve for (F^-) in mols/L.
You have 1.00 L so that is the number of mols F^- (= mols NaF) that must be added.
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