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K sp and the Solubility Product Constant

K sp and the Solubility Product Constant. K sp. The Solubility Product Constant The study of __________ _________ compounds. The Solubility Product Principle. CaF 2 Mg 3 (PO 4 ) 2 BaSO 4. Example 1.

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K sp and the Solubility Product Constant

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  1. Ksp and the Solubility Product Constant

  2. Ksp • The Solubility Product Constant • The study of __________ _________ compounds

  3. The Solubility Product Principle • CaF2 • Mg3(PO4)2 • BaSO4

  4. Example 1 • One liter of saturated barium sulfate solution contains 0.0025 g of BaSO4. What is the molar solubility of BaSO4? Calculate the Ksp.

  5. Example 2 • One liter of a saturated solution of silver chromate contains 0.0435 g of Ag2CrO4. Calculate the molar solubility and the solubility product constant.

  6. Example 3 • Calculate the molar solubilities, of the constituent ions, and total compound solubility of • Silver Chloride (Ksp = 1.8 x 10-10 • Zinc Hydroxide (Ksp = 4.5 x 10-17

  7. Calculate the molar solubility of MgF2 in pure water. • If it is placed in 0.1M NaF solution.

  8. Qsp vs. Ksp • If Qsp < Ksp then _____________________ • If Qsp = Ksp then solution ________________ • If Qsp > Ksp then ________________________

  9. If 100 ml of 0.00075M sodium sulfate is mixed with 50 ml of 0.015M barium chloride, will a precipitate form?

  10. What [Ba2+] is necessary to start the precipitation of BaSO4 in a solution that is 0.0015M in Na2SO4? Assume that the Ba2+ comes from addition of a solid soluble ionic compound such as BaCl2.

  11. Suppose we wish to recover silver from an aqueous solution that contains a soluble silver compound such as AgNO3 by precipitating insoluble silver chloride. A soluble ionic compound such as NaCl can be used as a source of Cl-1. What is the minimum concentration of chloride ion needed to reduce the dissolved silver ion concentration to a minimum of 1.0 x 10-9M?

  12. Fractional Precipitation • Solid silver nitrate is slowly added to a solution that is 0.0010M each in NaCl, NaBr, NaI. Calculate the [Ag+] required to initiate the precipitation of each of the silver halides.

  13. Based upon the before question, calculate the percentage of Iodine precipitated before AgBr precipitates. Calculate the percentages of Iodine and Bromine precipitated before Chlorine precipitates.

  14. Simultaneous Equilibria • If a solution is made of 0.10 M Magnesium Nitrate, and 0.10 M aqueous ammonia, will magnesium hydroxide precipitate?

  15. What concentration of aqueous ammonia is necessary to just start precipitation of Mg(OH)2 from a 0.10 M solution of Mg(NO3)2

  16. What is the molar solubility of Iron (III) Hydroxide in pure water? • What is it in a pH of 5.0 solution? • What is it in a pH of 13.0 solution?

  17. If a solution is made 0.080M Mg(NO3)2, 0.075M NH3, and 3.5 M NH4NO3, will Mg(OH)2 precipitate? What is the pH of this solution?

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