Concept:The solubility product (\( K_{sp} \)) is a specific type of equilibrium constant. Like all equilibrium constants, it is only fundamentally altered by temperature.
Solution:- Dissolution of a salt is either endothermic or exothermic.
- Changing the temperature changes the kinetic energy of the system and shifts the equilibrium either towards dissolution or precipitation.
- Because the fundamental ratio of equilibrium shifts, the actual constant \( K_{sp} \) changes.
- Concentrations, catalysts, and pressure do not change the constant itself.
Why other options are incorrect:Solvent changes the absolute solubility, but \( K_{sp} \) is defined for a specific solvent (usually water). Pressure rarely affects solids/liquids. Catalysts never change equilibrium constants.
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