79.2k views
0 votes
If Q (>/=/<) Ksp, the solution is saturated and no precipitation will occur. True/False

User Ben Dunlap
by
8.1k points

1 Answer

6 votes

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.

User Hbrls
by
8.3k points

No related questions found

Welcome to QAmmunity.org, where you can ask questions and receive answers from other members of our community.