A pure sample of strontium fluoride, SrF2, is introduced into distilled water at 25 °C. The solubility–product constant of SrF2 at this temperature is Ksp=2.5×10−9. A chemist wishes to prepare a saturated solution using exactly 250mL of water.
(a) Write the balanced chemical equation that represents the dissolution of SrF2 in water.
(b) Using the value of Ksp, calculate the molar solubility (in mol L−1) of SrF2 at 25 °C.
(c) Determine the maximum mass of SrF2 (in grams) that can completely dissolve in 250mL of water at 25 °C. Report your answer with the appropriate number of significant figures and units.