Lect+24+08 - Objectives for Solubility lecture Plain...

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Objectives for Solubility lecture Plain language understanding of dissolution Equilibrium (Solubility Product) Using the solubility product “K sp ” to calculate solubility A plain language understanding of the common ion effect Calculations of solubility with common ions present Plain language understanding and calculations of precipitation based on the solubility product Effects of pH on solubility
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Dissolution and Precipitation Equilibria EQUILIBRIUM: solid-gas analogous to diss/precip At equil: sublimation rate = solid deposition rate Volatile solid equilibrium vapor pressure in gas phase EQUILIBRIUM: solid-solution At equil: dissolution rate = solid precipitation rate Soluble solid equilibrium concentration in solution Saturated solution is in equilibrium with solid Unsaturated solution - solid is no longer present and excess solvent has been added (not in equilibrium) Supersaturated solution - concentration of dissolved solid exceeds the solubility product (not in equilibrium)
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Solubility depend on temperature Endothermic dissolution reactions generally displays increased solubility with increasing temperature What thermodynamic factor drives these endothermic dissolution reactions? Think G Exothermic reaction generally display decreased solubility with increasing temperature
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Classical Equilibrium Expressions - K sp For highly soluble salts (e.g. CsCl) the concentrated solutions which form are affected significantly by ion pairing and the saturated solutions formed are non-ideal. Classical equilibrium expressions of the type
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This note was uploaded on 04/01/2008 for the course CHEM 230 taught by Professor Sharp during the Winter '08 term at University of Michigan.

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Lect+24+08 - Objectives for Solubility lecture Plain...

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