CM1131_practical_3 - CM1131 Name: _ Lab Group: 1B Date:...

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Name: ________ Date: 31-Jan-07 Lab Group: 1B LAB REPORT E XPERIMENT 3 SOLUBILITY AND SOLUBILITY PRODUCT A IM To determine the solubility of KHC 4 H 4 O 6 in water and in 4 other solutions containing K + ions in different concentrations. To determine if the solubility product, K sp , is independent of the common ion concentration. I NTRODUCTION When dissolved in water, ionic compounds dissociate into their constituent ions in an equilibrium manner. KHC 4 H 4 O 6 (s) K + (aq) + HC 4 H 4 O 6 - (aq) At a particular temperature, the equilibrium constant for this dissociation will be the same. [ ][ ] } { ) ( ) ( ) ( 6 4 4 6 4 4 s aq aq O H HC K O H HC K K c - + = This reduces to a constant solubility product (since activity of solid = 1): [ ][ ] ) ( ) ( 6 4 4 aq O H HC aq K K sp - + = By Le Chatelier’s Principle, addition of common K + ions will shift the equilibrium to the left, however K c should remain constant, hence K sp should also not vary. K c and K sp only depend on temperature, as: RT G e K ° - = Through acid-base titration, this experiment seeks to investigate the claim that K sp is independent of concentration of K + ions, by adding KNO 3 to the potassium hydrogen tartate solution equilibrium to introduce common ions. 1
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CM1131_practical_3 - CM1131 Name: _ Lab Group: 1B Date:...

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