Problem: What is the solubility of CaF2 (assume Ksp = 4.0 x 10-11 ) in 0.030 M NaF?

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For this problem, we’re being asked to calculate the solubility of CaF2 in 0.030 M NaF?


Since the compounds are ionic compounds, they form ions when dissociating in water. The dissociation of CaFand NaF in water are as follows:


The chloride ion, F, has a charge of –1. Ca then has a charge of +2:

CaF(s)  Ca+(aq) + 2 F(aq)


The chloride ion, F, has a charge of –1. Na then has a charge of +1:

NaF (s)  Na+(aq) + F(aq)


Calculate the F- concentration in 0.030 NaF.

0.030 mol NaF1 L ×1 mol F-1 mol NaF

= 0.030 M F-


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Problem Details

What is the solubility of CaF2 (assume Ksp = 4.0 x 10-11 ) in 0.030 M NaF?

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What scientific concept do you need to know in order to solve this problem?

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