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Chemistry 18.3

Chemistry 18.3. Solubility Equilibrium. 18.3.

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Chemistry 18.3

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  1. Chemistry 18.3

  2. Solubility Equilibrium 18.3 • Barium sulfate is ingested by a patient before X-ray images of the digestive tract are taken. Barium sulfate absorbs the X-rays, thereby producing light areas on the developed X-ray film. However, barium salts are usually toxic. You will learn why patients can ingest this poisonous substance without harm.

  3. 18.3 The Solubility Product Constant • The Solubility Product Constant • What is the relationship between the solubility product constant and the solubility of a compound?

  4. 18.3 The Solubility Product Constant • The solubility product constant (Ksp), equals 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 the solubility product constant, the lower the solubility of the compound.

  5. 18.3 The Solubility Product Constant

  6. 18.3 The Solubility Product Constant

  7. 18.3 The Solubility Product Constant • Silver chloride is slightly soluble in water.

  8. 18.3 The Solubility Product Constant • Scale, formed by the precipitation of slightly soluble salts, builds up around faucets.

  9. 18.3

  10. 18.3

  11. 18.3

  12. 18.3

  13. for Sample Problem 18.3 Problem Solving 18.17 Solve Problem 17 with the help of an interactive guided tutorial.

  14. 18.3 The Common Ion Effect • The Common Ion Effect • How can you predict whether precipitation will occur when two salt solutions are mixed?

  15. 18.3 The Common Ion Effect • If the product of the concentrations of two ions in the mixture is greater than the Ksp of the compound formed from the ions, a precipitate will form.

  16. 18.3 The Common Ion Effect • A common ion is an ion that is found in both salts in a solution. The lowering of the solubility of an ionic compound as a result of the addition of a common ion is called the common ion effect.

  17. 18.3 The Common Ion Effect When a few drops of lead nitrate are added to the solution, more lead(II) chromate precipitates. A saturated solution of lead(II) chromate is pale yellow.

  18. 18.4

  19. 18.4

  20. 18.4

  21. 18.4

  22. for Sample Problem 18.4 Problem Solving 18.19 Solve Problem 19 with the help of an interactive guided tutorial.

  23. 18.3 Section Quiz. • 18.3.

  24. 18.3 Section Quiz. • 1. What is the concentration of a saturated solution of silver sulfide? • The Ksp of Ag2S is 8.0  10-51. • 2.0  10-17M • 8.9  10-26M • 8.9  10-25M • 2.0  1017M

  25. 18.3 Section Quiz. • 2. Adding which of these solutions to a saturated solution of BaSO4 will cause the solubility of BaSO4 to decrease? • I. BaCl2(aq) • II. Na2SO4 (aq) • (I) only • (II) only • (I) and (II) • neither solution

  26. 18.3 Section Quiz. • 3. The Ksp of AgBr is 5.0  10-13. When 7.1  10-6 mol/L solutions of NaBr(aq) and AgNO3(aq) are mixed, we would expect • no precipitate to form. • a definite precipitation reaction. • no reaction. • a saturated solution but no visible precipitation.

  27. 18.3 Section Quiz. • 4. After the common ion effect causes a precipitate to form in a solution, • the solution will no longer be saturated. • the solution will again be saturated. • the solution will be supersaturated. • there will be no solute left in the solution.

  28. END OF SHOW

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