Question

_____ occurs when the product of the ion concentrations exceeds the Ksp.

Answer 1

Precipitation occurs when the product of the ion concentration exceeds the Ksp.

Answer 2

Answer : Precipitation occurs when the product of the ion concentrations exceeds the $K__{sp}$.

Explanation :

Ionic product : It is the product of the concentrations of the ions in solution raised to the same power by its stoichiometric coefficient in a solution of a salt. This takes place at any concentration. The ionic product is represented as, Q.

Solubility product constant : It is defined as the product of the concentration of the ions present in a solution raised to the power by its stoichiometric coefficient in a solution of a salt. This takes place at equilibrium only. The solubility product constant is represented as, $K__{sp}$.

There are three cases for the solubility :

1. When $Q$ this means that the solution is unsaturated solution and more solid will be dissolve.
2. When $Q=k_{sp}$ this means that the solution is saturated solution.
3. When $Q>k_{sp}$ this means that the solution is supersaturated solution and solid will be precipitate.

Hence, the precipitation occurs when the product of the ion concentrations exceeds the $K__{sp}$.