If ionic product is less than Ksp then:
Correct answer: D. No precipitation will occur
- A. Solution will be saturated
- B. Precipitation will occur
- C. Solution will be super saturated
- D. No precipitation will occur
Explanation
Option D is correct. The ionic product is less than the solubility product, meaning the solution contains fewer ions than it could have at equilibrium. There is room for more ions and the saturation point is not reached. As saturation is not attained, therefore, precipitation does not occur. There are insufficient ions to exceed Ksp and form a solid precipitate. ==> Precipitation only occurs when the ionic product exceeds Ksp.
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About Solubility Product
The solubility product constant, Ksp, represents the equilibrium concentrations of ions from a sparingly soluble salt, each raised to its stoichiometric power. Problems involve writing Ksp expressions, calculating molar solubility, applying the common-ion effect and predicting precipitation from the ionic product.
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