Which of the following compounds, when dissolved in a 0.01...

Which of the following compounds, when dissolved in a 0.01 -M solution of HClO, has a solubility greater
than in pure water: $\mathrm{CuCl}$ , $\mathrm{CaCO}_{3}, \mathrm{MnS}, \mathrm{PbBr}_{2}, \mathrm{CaF}_{2} ?$ Explain your answer.

Key Concepts

Le Chatelier’s Principle

Le Chatelier’s Principle states that if a dynamic equilibrium system is disturbed by changing the conditions, the system responds by counteracting the change to re-establish equilibrium. In the context of sparingly soluble salts, if an acid reacts with one of the ions produced by the salt, the equilibrium shifts in the direction that supplies more of that ion, which enhances the solubility of the compound. This idea ties together the concepts of K_sp, the common ion effect, and acid-base reactions in solubility.

Acid-Base Reactions in Solubility Equilibria

Some sparingly soluble salts produce anions that are bases when dissolved in water. When such salts are in an acidic medium, the added hydrogen ions (H?) react with the basic anions to form weak acids, effectively reducing the concentration of free anions in solution. This reaction drives the dissolution equilibrium to favor further dissolution of the salt, thereby increasing its overall solubility compared to that in pure water.

Common Ion Effect

The common ion effect explains how the addition of an ion that is already part of the equilibrium of a sparingly soluble salt can shift the equilibrium. Typically, adding a common ion suppresses the solubility of the salt. However, if the ion released by the dissolving salt is also subject to a secondary reaction that removes it from the solution – such as by protonation – the equilibrium shifts in a way that increases the salt’s solubility.

Solubility Product (K_sp) and Equilibrium

This concept deals with the equilibrium that exists when a sparingly soluble ionic compound dissolves in water. The solubility product constant (K_sp) represents the product of the molar concentrations of the ions each raised to the power of its coefficient in the dissolution reaction. When a change in solution conditions shifts the established equilibrium, the solubility of the compound can increase or decrease in order to re?establish the equilibrium dictated by the K_sp value.

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