solubility product ksp
Overview
This lesson introduces the solubility product constant, Ksp, a crucial equilibrium constant used to describe the solubility of sparingly soluble ionic compounds. We will explore its definition, how to calculate it from solubility, and its applications in predicting precipitation and understanding common ion effects.
Introduction to Solubility and Ksp
Most ionic compounds are considered soluble, but even 'insoluble' salts dissolve to a very small extent. The solubility product constant, Ksp, quantifies this extent of dissolution for sparingly soluble ionic compounds. When such a compound, like silver chloride (AgCl), is added to water, an equilib...
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Key Concepts
- Solubility Product Constant (Ksp): An equilibrium constant that represents the product of the concentrations of the ions in a saturated solution of a sparingly soluble ionic compound, each raised to the power of its stoichiometric coefficient.
- Saturated Solution: A solution in which the maximum amount of solute has been dissolved at a given temperature, and any additional solute will not dissolve.
- Molar Solubility (s): The number of moles of solute that dissolve to form one liter of saturated solution, typically expressed in mol dm⁻³.
- Sparingly Soluble Salt: An ionic compound that dissolves to a very small extent in water, forming a saturated solution with low ion concentrations.
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Exam Tips
- →Always write out the balanced dissolution equation and the correct Ksp expression for the given salt. Pay close attention to the stoichiometric coefficients as they become exponents in the Ksp expression.
- →Clearly define 's' (molar solubility) and relate it to the equilibrium concentrations of the ions using the stoichiometry of the reaction. For example, for CaF₂, if solubility is 's', then [Ca²⁺] = s and [F⁻] = 2s.
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