🤓 Based on our data, we think this question is relevant for Professor Dixon's class at UCF.
We are asked to calculate the solubility product constant, Ksp, for CaF2 at a certain temperature, 35°C, given its molar solubility (1.24x10-3 mol/L).
Recall that Ksp measures how soluble the compound will be in a solvent. In this case, we use the universal solvent, water, as it is not specified in the problem.
If the molar solubility of CaF2 at 35°C is 1.24 x 10-3 mol/L, what is the Ksp at this temperature?