Lecture 22 - Lecture 22: Solubility Product Constants...

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Lecture 22: Solubility Product Constants Recall that when we defined activities, we stated that the activity of a solid equals unity. The solubility product constant (Ksp) is simply the equilibrium constant for a solid as a reactant forming dissolved species as products. General example: AB(solid) A+ + B- (in solution) The most popular high school chemistry experiments are based on this kind of equilibrium! Very often, the reactions are done in reverse; soluble species are mixed and solids appear when the concentrations in the solution are much higher than allowed by the solubility product constants. The solids that come out are the ones with the LOWEST Ksp. The ions left behind would form solids that have higher Ksp. By weighing the amounts of the precipitated solids, one can deduce how much of a particular ion was originally in the solution, if it is all converted to some insoluble solid. Well known example: adding excess chloride to silver nitrate---all the silver forms silver chloride solid. For an ionic solid, the species in solution are NOT molecules of the formula unit of the solid. They are individual ionic species with their own individual activities that appear
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This note was uploaded on 09/29/2009 for the course ME 530.230 taught by Professor Katz during the Spring '09 term at Johns Hopkins.

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Lecture 22 - Lecture 22: Solubility Product Constants...

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