Lead(II) iodide is only slightly soluble in water. At 60 °C, 0.0410 g of PbI₂ dissolves in exactly 100.0 mL of water to produce a saturated solution while excess solid remains. The formula mass of PbI₂ is 461.0 g mol⁻¹.
(a) Calculate the molar solubility of PbI₂ at 60 °C.
(b) Using appropriate stoichiometric relationships, determine the concentrations of Pb²⁺ and I⁻ ions present at equilibrium.
(c) Compute the numerical value of the solubility-product constant for PbI₂ at 60 °C.
(d) A chemist adds solid NaI to this saturated solution until the iodide-ion concentration reaches 0.15 M at 60 °C. Predict whether additional PbI₂ will precipitate, and justify your answer with a calculation.