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Chemistry 122

Chemistry 122. Solubility Equilibrium. The Solubility Product Constant. Solubility varies from one ionic compound to the next Some ionic compounds can dissolve quite significantly in water where others cannot They are either soluble or insoluble

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Chemistry 122

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  1. Chemistry 122 Solubility Equilibrium

  2. The Solubility Product Constant • Solubility varies from one ionic compound to the next • Some ionic compounds can dissolve quite significantly in water where others cannot • They are either soluble or insoluble • Table 18.1, p. 561 highlights some of the solubilities of various ionic compounds • Water is always the solvent

  3. Ksp – continued… • Although an ionic compound may be considered insoluble, a small amount does actually dissolve • The equilibrium reaction would be as follows: Ionic Compound(s)↔ Cation+(aq) + Anion-(aq) AgCl(s)↔ Ag1+(aq) + Cl1-(aq)

  4. Ksp – continued… The equilibrium expression is written as follows: Keq = [Ag1+] x [Cl1-] [AgCl] • As long as some undissolved solid is present, the concentration remains the same; it is a constant • Therefore, the concentration of undissolved solid can be combined with Keq since it, too, is a constant

  5. Ksp – continued… Keq x [undissolved solid] = [cation] x [anion] = Ksp • This new constant, Ksp, is called the solubility product constant • It is equal to the product of the concentrations of the ions each raised to a power equal to the coefficient of the ion in the dissociation equation • The smaller the numerical value of Ksp, the lower the solubility of the compound

  6. Summary Any ionic solid placed in water establishes an equilibrium between its dissociated ions in solution and the solid that is undissolved. The solubility product constant is an equilibrium constant that describes the equilibrium between a solid and its ions in solution. Table 18.2, p. 562 – examine for high/low solubilities.

  7. Finding Ion Concentrations in a Saturated Solution When Ksp is given, the ion concentration of either the cation or anion can be found Sample Problem 18.3 What is done to overcome the problem of not knowing either ion concentration? Questions 17, 18, p. 562.

  8. One More Problem What is the concentation of barium and sulfate ions in a saturated barium sulfate solution at 25°C? Ksp = 1.1 x 10-10

  9. The Common Ion Effect • When an ionic compound has reached saturation, another ionic compound can be added to increase the concentration of one of the ions • LeChatelier'sprinciple says that when a stress is applied to an equilibrium, it re-establishes itself by adjusting its equilibrium position • The reaction will shift to the left, resulting in more reactant (ionic compound(s)) forming

  10. Common Ion Effect – continued… • As long as another compound, containing either a cation or anion from the original compound, is being added, the equilibrium position will adjust itself so that Kspdoes not change Original – Ksp= [Pb2+] [CrO42-] = 1.8 x 10-14 • Adding Pb(NO3)2 Revised – Ksp = [Pb2+][CrO42-] = 1.8 x 10-14

  11. Definitions • A common ion is the cation or anion that is found in both ionic compounds (salts) in a solution • Common ion effect is the lowering of the solubility of an ionic compound as a result of the addition of a common ion • Spectator ions are those that do not participate in the reaction. They stay in solution and do not precipitate

  12. Precipitates • Kspcan be used to determine whether a precipitate will form when solutions are mixed • If the product of the concentration of two ions (Qsp) in the mixture is greater than the Ksp of the compound formed from the ions, a precipitate will form

  13. Example Ex. Ksp of BaSO4 = 1.1 x 10-10 Ba(NO3)2 = 0.50L, 0.002M Na2SO4 = 0.50L, 0.008M Possible precipitate = Ba(SO4)2 The product of the ions barium and sulfate has to exceed the Ksp Because they are mixed, the concentrations are cut in half, so…

  14. Precipitate Example… Ba(NO3)2 = 0.001M (mol/L) Na2SO4 = 0.004M (mol/L) [Ba2+] = 0.001M [SO42-] = 0.004M Qsp = [Ba2+] x [SO42-] =(0.001M) x (0.004M)=4 x 10-6 Ksp = 1.1 x 10-10Does a precipitate form?

  15. Finding Equilibrium Ion Concentration Using a Common Ion Work through Sample Problem 18.4, p. 564. Questions 19, 20, p. 564 Questions 21 – 28, p. 565 Section 18.3 Review

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