Concept:The relationship between the ionic product (\( Q_{sp} \)) and the solubility product (\( K_{sp} \)) determines whether a solution is unsaturated, saturated, or supersaturated.
Formula:$$ \text{If } Q_{sp} > K_{sp} \implies \text{Precipitation} $$
Solution:- \( Q_{sp} \) represents the actual product of ion concentrations in a solution at any given moment.
- When \( Q_{sp} > K_{sp} \), the solution contains more dissolved ions than it can stably hold at equilibrium (supersaturated).
- To restore equilibrium, the excess ions precipitate out as a solid until \( Q_{sp} \) drops down to equal \( K_{sp} \).
Why other options are incorrect:Less than \( K_{sp} \) means the solution is unsaturated (no precipitation). Equal to \( K_{sp} \) means it is perfectly saturated (equilibrium, no net precipitation).
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