Solubility Equilibria Of Sparingly Soluble Salts

• Solution A (pH = 6.0): [H⁺] = 10^-6 M
• Solution B (pH = 4.0): [H⁺] = 10^-4 M

We are given the compounds AgCl, NaCl, and CaCl₂ in various solvents.

To determine the order of solubility, consider the following:

- AgCl is sparingly soluble in water, but the presence of ions like NaCl or CaCl₂ can reduce its solubility due to the common ion effect.

- CaCl₂ dissociates into Ca²⁺ and Cl^- ions, which can shift the equilibrium and increase the solubility of AgCl.

- NaNO₃ does not participate in the common ion effect and will have minimal interference with the solubility of AgCl.

Therefore, the increasing order of solubility is: