Final answer:
AgBr is the compound with a solubility greater than in pure water when dissolved in a 0.01-M solution of HClO4. Therefore, the compound with potentially increased solubility in the acidic solution is option d) PbI₂.
Step-by-step explanation:
In a 0.01-M solution of perchloric acid (HClO₄), the ion concentrations are elevated compared to pure water due to the dissociation of the acid. To determine which compound has increased solubility in this acidic solution, we can consider the solubility rules.
a) AgBr: Silver bromide (AgBr) is insoluble in water, and the addition of HClO₄ would not significantly increase its solubility.
b) BaF₂: Barium fluoride (BaF₂) is sparingly soluble in water, and the acidic solution is not expected to greatly enhance its solubility.
c) Ca₃(PO₄)₂: Calcium phosphate (Ca₃(PO₄)₂) is generally insoluble, and the acidic solution is unlikely to significantly alter its solubility.
d) PbI₂: Lead iodide (PbI₂) is sparingly soluble in water, and the presence of HClO₄ might increase its solubility due to the formation of soluble Pb²⁺ ions.
Therefore, the compound with potentially increased solubility in the acidic solution is option d) PbI₂.