13_LectureWeb - Learning Objectives 2/21/08 You should: 1....

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Learning Objectives 2/21/08 You should: 1. know how to calculate decreases in the solubility of ionic compounds resulting from the common ion effect . 2. be able to predict how changes in pH will affect the solubility of ionic compounds. 3. understand why complex ion formation enhances the solubility of ionic compounds and know how to determine the solubility of an ionic compound in the presence of a complexing agent. Common Ion Effect The solubility of a salt will decrease in the presence of a common ion (one of the ionic participants in the solubility equilibrium). Consider the insoluble salt SrF 2 SrF 2 H s L F Sr 2 + H aq L + 2F - H aq L Addition of the soluble salt NaF (F - is the common ion) will suppress the dissolution of SrF 2 . According to LeChatelier’s Principle, addition of one of the products in the equilibrium reaction will shift equilibrium toward reactants reducing the amount of SrF 2 dissolved. 2 In the previous lecture we calculated the solubility of SrF 2 and found that it was 8.6 ä 10 - 4 M. Find the solubility of SrF 2 in a solution that also contains 0.1 M of the soluble salt NaF. K
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This note was uploaded on 03/19/2008 for the course CEM 142 taught by Professor A.pollock during the Spring '08 term at Michigan State University.

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13_LectureWeb - Learning Objectives 2/21/08 You should: 1....

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