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Ch 17.4 Notes - filled in

by: lucy farrar

Ch 17.4 Notes - filled in CHEM 1202

Marketplace > Louisiana State University > Chemistry > CHEM 1202 > Ch 17 4 Notes filled in
lucy farrar
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Ch 17.4 notes with all class notes and example problems
Chem 1202
Class Notes
Chem, chem 1202, 1202, Chemistry
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This 9 page Class Notes was uploaded by lucy farrar on Sunday January 31, 2016. The Class Notes belongs to CHEM 1202 at Louisiana State University taught by Hurst in Spring 2016. Since its upload, it has received 38 views. For similar materials see Chem 1202 in Chemistry at Louisiana State University.


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Date Created: 01/31/16
Chapter 17 Section 4 Solubility Equilibria Suggested Problems: 51, 52, 53, 54, 55, 56 17.4 Solubility Equilibria Solubility equilibria are those that involve the dissolution or precipitation of ionic compounds. These reactions are heterogeneous. We know the general rules for predicting the solubility of common salts in water, which is only qualitative. By using solubility equilibria we can make quantitative predictions about the solubility. 17.4 Solubility Equilibria 2+ 2- BaSO (4) Ba (aq) + SO 4 (aq) A saturated solution will be formed when the solution is in contact with undissolved solute. The extent to which the dissolution reaction occurs is expressed by the magnitude of the solubility-product constant (Ksp. 2+ 2- K sp[Ba ] [SO ] 4 17.4 Solubility Equilibria Do not confuse the solubility of a substance with the solubility-product constant (K ).sp The solubililty of a substance is the quantity that dissolves to form a saturated solution and is usually given in g/L or mol/L. The K sp the equilibrium constant for the equilibrium between and ionic solid and its saturated solution. BaSO (s) Ba (aq) + SO 2-(aq) ionic solid saturated solution 17.4 Solubility Equilibria AgCl (s) Ag + Cl - K = 1.8 x 10 -10 sp + - -13 AgBr (s) Ag + Br Ksp 5.0 x 10 AgI (s) Ag + I - Ksp 8.3 x 10 -17 Hint: K << 1, reactants predominate 17.4 Solubility Equilibria Calculating K fspm Solubility Calculate the K ospAg CrO2(s) 4f at equilibrium the concentration of Ag 1.3x10 M. -4 17.4 Solubility Equilibria Calculating Solubility from K sp The K sprm CaF is 329 x 10 -11at 25 °C. Assuming that CaF dissociates completely upon dissolving, calculate 2 the solubility of CaF 2n grams per liter.


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