Final answer:
The salts AgCN, ZnS, Zn₃(PO₄)₂ (zinc phosphate), CaCO₃ (calcium carbonate), and BiI₃ are substantially more soluble in acidic solutions than in pure water. This increased solubility is due to the reaction between the acidic protons and the anions of the salts, which forms products that are either gaseous and escape from the solution or remain as a weak acid, thereby reducing the anion concentration and tipping the equilibrium towards more salt dissolving.
Step-by-step explanation:
Salts that are substantially more soluble in acidic solution than in pure water are often salts of weak bases and strong acids, as the acidic solution can react with the anions of the salt, effectively removing them from the equilibrium and shifting it to dissolve more of the solid salt. In this scenario, the salts that will be more soluble in acidic solution than in pure water are:
- AgCN (Silver cyanide): AgCN dissolves in acid because the CN− ion will react with H+ to form HCN gas, which leaves the solution.
- ZnS (Zinc sulfide): The S^2− ions from ZnS can react with H+ to form H2S gas, thus increasing the solubility of ZnS in acidic solutions.
- Zn₃(PO₄)₂ (Zinc phosphate): The PO4^3− ions can react with acids to form HPO4^2− or H2PO4−, depending on the pH, enhancing the solubility of zinc phosphate in acid.
- CaCO₃ (Calcium carbonate): Acid can react with the CO3^2− ions to form HCO3− or CO2 and H2O, which increases the solubility of calcium carbonate in acidic solution.
- BiI₃ (Bismuth iodide): The I− ions react with H+ to form HI, which is less soluble and may leave the solution as a gas or remain as a weak acid. This can enhance the solubility of BiI₃ in an acidic solution.