CHEM 104 Lecture Notes - Lecture 26: Solubility Equilibrium, Ionic Compound, Equilibrium Constant
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Ex: fe2s3 (s) 2fe3+ (ag) + 3s2- (ag) * solubility and solubility product constant are not the same thing * Solubility = the amount of solute per unit volume of solution (mol/l) that dissolved to form a saturated solution. Solubility product constant = the equilibrium constant for the chemical equilibrium that exists between a solid ionic solute and its ions in a saturated solution. Ex: ag+ and cl- = 6. 3 x 10-6 m. Ksp = [ag+] [cl-] = [6. 3 x 10-6] [6. 3 x 10-6] = 4. 0 x 10-11. * this process may seem straightforward to calculate the solubility of an ionic compound from its ka. * ionic salts such as pbcl2 dissociate stepwise, so that pbcl+ ions as well as pb2+ and cl- ions are present. * ion pairs, such as pbcl+ cl- can exist, reducing the concentrations of unassociated. * the solubilities of some solutes, such as metal hydroxides, depend on the acidity or alkalinity of the solution.
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