Ksp: The solubility product constant, an equilibrium constant. Qsp: The ion product, calculated using initial concentrations to predict precipitation.

The extent to which a substance dissolves in a solvent, reaching an equilibrium between the solid and its ions in solution.

The solubility product constant; the equilibrium constant for the dissolution of a solid in a solution.

A highly soluble compound; the dissolution reaction proceeds far to the right.

A poorly soluble compound; the dissolution reaction barely proceeds to the right.

The concentration of the metal cation in a saturated solution.

The ion product is a measure of the relative amount of ions in a solution. It predicts whether a precipitate will form.

1. Write the dissolution reaction. 2. Convert solubility from g/L to mol/L (Molarity). 3. Plug molarity into the Ksp expression: Ksp = [ion1]^coefficient * [ion2]^coefficient.

1. Write the dissolution reaction. 2. Set up a RICE table. 3. Plug equilibrium concentrations (in terms of 'x') into the Ksp expression. 4. Solve for 'x', which represents the molar solubility.

1. Calculate Qsp using initial ion concentrations. 2. Compare Qsp to Ksp: If Qsp > Ksp, precipitation occurs. If Qsp < Ksp, no precipitation occurs. If Qsp = Ksp, the solution is at equilibrium.