Final answer:
The statement is true when Q equals Ksp, indicating a saturated solution in equilibrium where no precipitation occurs.
Step-by-step explanation:
The relationship between Q (the reaction quotient) and Ksp (the solubility product constant) determines the solubility state of a solution. If Q = Ksp, the solution is saturated and no further precipitation will occur because the rates of dissolution and precipitation are equal, and the solution is at equilibrium. Therefore, the statement 'If Q (>/=/<) Ksp, the solution is saturated and no precipitation will occur' is true when Q equals Ksp. This equilibrium state is where the dissolved ions in the solution are in a dynamic balance with the solid phase, and any additional solid added to the solution will not dissolve.