Concept of Solubility Equilibria of Sparingly Soluble Salts

The solubility product constant of Ag₂CrO₄ and AgBr are 1.1 × 10^–12 and 5.0 × 10^–13respectively. Calculate the ratio of the molarities of their saturated solutions.

Equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together. Will it lead to precipitation of copper iodate? (For cupric iodate K_sp = 7.4 × 10^–8).

A sparingly soluble salt gets precipitated only when the product of concentration of its ions in the solution (Q_sp) becomes greater than its solubility product. If the solubility of \[\ce{BaSO4}\] in water is 8 × 10^–4 mol dm^–3. Calculate its solubility in 0.01 mol dm^–3 of \[\ce{H2SO4}\].

The solubility product of \[\ce{Al(OH)3}\] is 2.7 × 10^–11. Calculate its solubility in gL^–1 and also find out pH of this solution. (Atomic mass of \[\ce{Al = 27 u}\]).

A sparingly soluble salt having general formula \[\ce{A^{p+}_x B^{q-}_y}\] and molar solubility S is in equilibrium with its saturated solution. Derive a relationship between the solubility and solubility product for such salt.