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SOLUBILITY PRODUCT

SOLUBILITY PRODUCT. Presentation on. Insoluble salts are describe as sparingly soluble. A sparingly soluble salts dissolves to a small extent.

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SOLUBILITY PRODUCT

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  1. SOLUBILITYPRODUCT Presentation on

  2. Insoluble salts are describe as sparingly soluble. A sparingly soluble salts dissolves to a small extent. The solubility product is the new constant formed when the constant (Kc) multiplied by the concentration of the salt at a given temperature.

  3. Let AxBy represent a sparingly soluble salt At equilibrium; For a saturated solution of ionic solid in water: AxBy(s) xAy+(aq) + yBx-(aq)

  4. The new constant form from the product of constants Kc and AxBy(s) is Ks.p.. • Ks.p. represents the solubility product of the sparingly soluble salt AxBy(s).

  5. Example A Saturated solution of silver chloride contains 1.46 10-3 gdm-3 at 18°C. What is the solubility product of silver chloride at this temperature?

  6. LIMITIONS OF THESOLUBILITY PRODUCT CONCEPT(Ks.p.)

  7. Ksp is valid only for saturated solution in which the total concentration of the ions is no more than 0.01 mol dm-3. • Ksp is affected by temperature since it is an equilibrium constant.

  8. THE COMMON ION EFFECT.

  9. In the presence of either Ay+ or Bx- from a second source, the solubility of the salt AxBy is reduced known as Le Chatalier’s principle. • The common ion effect is the precipitation of a solute on addition of another solution which has an ion in common with the solute.

  10. Example • There is disruption in the equilibrium system but the(Ksp) would remain constant upon the addition of sodium sulphate to saturated solution of BaSO4(s). • BaSO4(s) Ba2+(aq) + SO2-4(aq) • NaSO4(s) 2Na+(aq) + SO2-4(aq)

  11. There would be an increase in the SO2-4 ions concentration due to the addition of NaSO4(s) to the BaSO4(s). • The Ksp would remain constant due to the increase of SO2-4 ions consequenting in a decrease in Ba2+(aq) ions concentration. • Thus the equilibrium would shift and the reduction of BaSO4 would occur.

  12. PREDICTING PRECIPITATION

  13. Ionic product < Ks.p, , no precipitation occurs. • Ionic product = Ks.p. , a saturated solution forms. • Ionic product > Ks.p. , precipitation occurs.

  14. Hence Kc = [Ay+(aq)]x [Bx-(aq)]y [AxBy(s)] [Kc][AxBy(s)] = [Ay+(aq)]x [Bx-(aq)]y Ks.p. = [Ay+(aq)]x [Bx-(aq)]y

  15. The solubility of silver chloride at 18°C = 1.46 10-3 g dm-3 = 1.46 10-3 143.5 mol dm -3 = 1 10 -5 mol dm -3

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