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Ch 8 - Effect of Ionic Strength on Solubility of Salts...

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Chapter 8 Activity Dr. E. Binamira-Soriaga Department of Chemistry Texas A&M University Effect of Ionic Strength on Solubility of Salts Hg 2 (IO 3 ) 2 (s) Hg 2 2+ (aq) + 2IO 3 (aq) K sp = [Hg 2 2+ ][IO 3 ] 2 = 1.3 x 10 -18 [IO 3 ] = 2[Hg 2 2+ ] K sp = [Hg 2 2+ ][2Hg 2 2+ ] 2 = 1.3 x 10 -18 [Hg 2 2+ ] = 6.9 x 10 -7 M (solubility in distilled water) Hg 2 (IO 3 ) 2 (s) Hg 2 2+ (aq) + 2IO 3 (aq) KNO 3 (s) K + (aq) + NO 3 (aq) [Hg 2 2+ ] = 1.0 x 10 -6 M (solubility in 0.05 M KNO 3 ) Effect of Ionic Strength on the Equilibrium Constant Fe 3+ (aq) + SCN (aq) Fe(SCN) 2+ (aq) K = [Fe(SCN) 2+ ]/ [Fe 3+ ][SCN ] Effect of Ionic Strength Ionic atmosphere decreases attraction between ions Greater ionic strength, higher charge on ionic atmosphere, lesser attraction between cation and anion Solubility of salt is increased Effect of Ionic Strength on Solubility of Potassium Tartrate Evaluation of Ionic Strength Ionic strength, μ , is a measure of the total concentration of ions in solution c i is the concentration of ith species Z i is the charge of the species Sum is over ALL ions in solution
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Evaluation of Ionic Strength Salts with +1 charged ions dissociate almost completely at concentrations < 0.1 M. For salts
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