A newly synthesized salt, ZrO₂Cl₂, dissolves according to
ZrO₂Cl₂(s) ⇌ ZrO²⁺(aq) + 2 Cl⁻(aq)
Its measured solubility–product constant at 25 °C is Ksp=0.80. In a laboratory test, however, a student observes that placing excess ZrO₂Cl₂ in 1.0 L of pure water produces a saturated solution containing 1.1mol of Cl⁻ ions.
(a) Before any measurements are performed, predict qualitatively whether ZrO₂Cl₂ should be classified as soluble, sparingly soluble, or effectively insoluble in water at 25 °C. Base your prediction solely on the magnitude of its Ksp.
(b) Using the observed chloride concentration, calculate the experimental molar solubility of ZrO₂Cl₂ under the test conditions.
(c) Compare the experimental result from part (b) with the qualitative prediction from part (a). Discuss at least two plausible chemical factors—grounded in equilibrium principles—that could account for any discrepancy between prediction and observation.