23-24 SolubilityLandscape - SOLUBILITY Solubility: quantity...

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CH112 LRSVDS SOLUIBILITY 1 SOLUBILITY Solubility: quantity of a substance that dissolves to form a _______________________ Units of Solubility: g/L Units of Molar solubility: mole/L Some salts are very soluble (> 0.1 M). Recall solubility rules. Some salts are sparingly soluble (< 0.1 M) sometimes referred to as ‘insoluble’. Precipitation and Solubility of ionic salts is an equilibrium in water MA(s) M + (aq) + A - (aq) CH112 LRSVDS SOLUIBILITY 2 SOLUBILITY EQUILIBRIA Precipitation: Dissolution: When the forward rate = backward rate: ______________! AgCl (s) Ag + (aq) + Cl - (aq) The concentration of solid does not change at equilibrium K sp = Solubility Product
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CH112 LRSVDS SOLUIBILITY 3 AgCl 1.8 x 10 -10 AgBr 5.0 x 10 -13 AgI 8.3 x 10 -17 CdS 8.0 x 10 -27 ZnS 1.1 x 10 -21 Mg(OH) 2 1.8 x 10 -11 Ca(OH) 2 5.5 x 10 -6 CaF 2 3.9 x 10 -11 BaCO 3 5.1 x 10 -9 BaSO 4 1.1 x 10 -10 SOLUBILITY PRODUCTS K sp CH112 LRSVDS SOLUIBILITY 4 SOLUBILITY CALCULATIONS Calculate [Ca 2+ ] and [F - ] for a saturated CaF 2 solution. 1) Write the reaction: CaF 2 (s) Ca +2 (aq) +2F - (aq) 2) Make an ice table 3) Write the equilibrium expression K sp = [Ca 2+ ][F - ] 2 =3.9 x 10 -11 at 25 o C 4) What is the solubility ? solubility = amount of salt dissociated
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CH112 LRSVDS SOLUIBILITY 5 Solubility and the COMMON ION EFFECT Add Ag + to solution at equilibrium; solubility _____ Add Cl - to solution at equilibrium; solubility _____ Add AgCl(s) to solution at equilibrium; solubility _____ AgCl (s) Ag + (aq) + Cl - (aq ) Addition of a Common Ion __________________ solubility
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This note was uploaded on 01/18/2012 for the course CHEM 112 taught by Professor Vandersluys,lorschmid,kylem during the Fall '07 term at Pennsylvania State University, University Park.

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23-24 SolubilityLandscape - SOLUBILITY Solubility: quantity...

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