Final answer:
If Q is greater than Ksp, the solution is supersaturated and a precipitate will form until equilibrium is reached. No precipitation occurs if Q is less than Ksp because the solution is unsaturated. When Q equals Ksp, the solution is saturated and at equilibrium.
Step-by-step explanation:
The solution to whether a precipitate will form depending on the relationship between Q (the reaction quotient) and Ksp (the solubility product constant) is indeed tied to their comparative values. If Q > Ksp, the solution is supersaturated, which means it contains more dissolved ions than it can ideally hold at equilibrium. In this situation, the surplus ions will form a precipitate until equilibrium is reached. On the contrary, if Q < Ksp, the solution is unsaturated and has the capacity to dissolve more of the solid without any precipitation occurring. When Q = Ksp, the system is at equilibrium, indicating a saturated solution where no further precipitation or dissolution occurs.