CaF2(s) will break up into its ions: CaF2(s) ⇌ Ca2+(aq) + 2 F-(aq)
Ca(NO3)2(s) also break up to its ions: Ca(NO3)2(s) ⇌ Ca2+(aq) + 2 NO3-(aq)
There is now an initial concentration of Ca2+ from Ca(NO3)2(s): this is called the Common Ion Effect
[Ca(NO3)2] = [Ca2+] = 0.55 M
Set up an ICE Table: CaF2(s) ⇌ Ca2+(aq) + 2 F-(aq)
Substitute equilibrium concentrations and solve for x:
Calculate the molar solubility of CaF2 in a solution containing 0.550 M of Ca(NO3)2. The Ksp value for CaF2 is 1.46 x 10–10.
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