Which of the following salts will be substantially more soluble in acidic solution than in pure water: (a) ZnCO3, (b) ZnS, (c) BiI3, (d) AgCN, (e) Ba3(PO4)2?

Verified step by step guidance

1. Identify the salts that contain anions which can react with H+ ions in an acidic solution. These anions typically come from weak acids.
2. Consider the solubility equilibrium of each salt in water and how the presence of H+ ions can shift this equilibrium by reacting with the anion.
3. For each salt, write the dissolution reaction and the possible reaction of the anion with H+ ions. For example, for ZnCO3, the dissolution reaction is ZnCO3(s) ⇌ Zn²⁺(aq) + CO₃²⁻(aq), and CO₃²⁻ can react with H+ to form HCO₃⁻ or H₂CO₃.
4. Evaluate which anions form weak acids upon reacting with H+ ions, as this will increase the solubility of the salt in acidic solution. For instance, CO₃²⁻ forms H₂CO₃, a weak acid, which increases the solubility of ZnCO3 in acidic solution.
5. Determine which salts have anions that form weak acids, making them more soluble in acidic solutions compared to pure water.