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Question
A saturated solution, prepared by dissolving CaF2(s) in water, has [Ca2+] = 3.3 × 10−4 M What is the Ksp of CaF2?
Solution
\[\ce{CaF2_{(s)} ⇌ Ca^{2+}_{( aq)} + 2F^-_{( aq)}}\]
[F−] = 2 [Ca2+]
= 2 × 3.3 × 10−4 M
= 6.6 × 10−4 M
Ksp = [Ca2+] [F−]2
= (3.3 × 10−4) (6.6 × 10−4)2
= 1.44 × 10−4
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