If ionic product becomes greater than solubility product, what will be the result?
Answer and explanation
Correct answer: Precipitate will form
The ionic product Q is calculated from the current ion concentrations, whereas Ksp describes the equilibrium limit for a saturated solution. If Q exceeds Ksp, the solution contains more ions than can remain dissolved at equilibrium. The excess ions combine to form solid until Q falls to Ksp. Therefore precipitation occurs; the solution is not unsaturated and neither solvent destruction nor gas formation follows.
Frequently asked questions
What is the correct answer to this question?
Precipitate will form
Why is this the correct answer?
The ionic product Q is calculated from the current ion concentrations, whereas Ksp describes the equilibrium limit for a saturated solution. If Q exceeds Ksp, the solution contains more ions than can remain dissolved at equilibrium. The excess ions combine to form solid until Q falls to Ksp. Therefore precipitation occurs; the solution is not unsaturated and neither solvent destruction nor gas formation follows.
Which subject and chapter does this question cover?
This is a Class 11 Chemistry question. Chapter: Equilibrium. Topic: Solubility product and common ion effect.
