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Unit 7 - Chpt 16 - Solubility equilibria and Quantitative analysis

Unit 7 - Chpt 16 - Solubility equilibria and Quantitative analysis. Solubility equilibria and Ksp Predict precipitation Qualitative analysis HW set1: Chpt 16 - pg. 766-771 # 19, 21, 23, 28, 33, 40, 43, 45, 50 - Due Tues. Mar 23

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Unit 7 - Chpt 16 - Solubility equilibria and Quantitative analysis

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  1. Unit 7 - Chpt 16 - Solubility equilibria and Quantitative analysis • Solubility equilibria and Ksp • Predict precipitation • Qualitative analysis • HW set1: Chpt 16 - pg. 766-771 # 19, 21, 23, 28, 33, 40, 43, 45, 50 - Due Tues. Mar 23 • Rev Problems: Chpt 16 - pg. 766-771 # - 25, 35, 56 Due Friday Mar 26

  2. Solubility Equilibria • Solubility product (Ksp) – equilibrium constant; has only one value for a given solid at a given temperature. • Solubility – an equilibrium position. Bi2S3(s) 2Bi3+(aq) + 3S2–(aq)

  3. Ksp values for some compounds

  4. Ksp Calc - examples Calculate the solubility of silver chloride in water. Ksp = 1.6 × 10–10 1.3×10-5M Calculate the solubility of silver phosphate in water. Ksp = 1.8 × 10–18 1.6×10-5M

  5. Solubility in acid sol’n - 1 How does the solubility of silver chloride in water compare to that of silver chloride in an acidic solution (made by adding nitric acid to the solution)? Explain. The solubilities are the same.

  6. Solubility in acid sol’n - 2 How does the solubility of silver phosphate in water compare to that of silver phosphate in an acidic solution (made by adding nitric acid to the solution)? Explain. The silver phosphate is more soluble in an acidic solution.

  7. Solubility in other salt sol’ns Calculate the solubility of AgCl (Ksp = 1.6 × 10–10) in: • 100.0 mL of 4.00 x 10-3Mcalcium chloride. 2.0×10-8M • 100.0 mL of 4.00 x 10-3Mcalcium nitrate. 1.3×10-5M

  8. Precipitation(Mixing 2 Solutions of Ions) • Q > Ksp; precipitation occurs and will continue until the concentrations are reduced to the point that they satisfy Ksp. • Q < Ksp; no precipitation occurs.

  9. Precipitation? Flow chart for solving Precipitation questions

  10. Selective Precipitation(mixtures of metal ions) • Use a reagent whose anion forms a precipitate with only one or a few of the metal ions in the mixture. • Example: • Solution contains Ba2+ and Ag+ ions. • Adding NaCl will form a precipitate with Ag+ (AgCl), while still leaving Ba2+ in solution.

  11. More soluble? • Two strategies for dissolving a water–insoluble ionic solid. • If the anion of the solid is a good base, the solubility is greatly increased by acidifying the solution. • In cases where the anion is not sufficiently basic, the ionic solid often can be dissolved in a solution containing a ligand that forms stable complex ions with its cation.

  12. Concept check (not covered for test) Calculate the solubility of silver chloride in 10.0 M ammonia given the following information: Ksp (AgCl) = 1.6 x 10–10 Ag+ + NH3 AgNH3+K = 2.1 x 103 AgNH3+ + NH3 Ag(NH3)2+K = 8.2 x 103 0.48 M Calculate the concentration of NH3 in the final equilibrium mixture. 9.0 M

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