A chemist is studying the behavior of three sparingly soluble salts when a strong acid is added to the solution.
• Salt X: CaF2
• Salt Y: SrCO3
• Salt Z: AgCl
Assume identical masses of each salt are separately stirred into 100mL of 0.10M HCl at 25∘C. The temperature is held constant and the mixtures are allowed to reach equilibrium.
(a) Rank the three salts from highest to lowest expected molar solubility under the acidic conditions described.
(b) Explain the chemical reasoning that leads to the ranking in part (a). Your answer should include discussion of any relevant equilibria and species present in solution.
(c) Qualitatively describe how the ranking in part (a) would change, if at all, when the experiment is repeated in pure water at the same temperature. Justify your response.