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More Ksp

More Ksp. Comparing Solubilities. The relative solubilities can be deduced by comparing values of K sp . BUT, BE CAREFUL! These comparisons can only be made for salts having the same ION:ION ratio. Comparing Solubilities. Which salt is more soluble? Ag 2 S Ksp = 1.0 X 10 -49

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More Ksp

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  1. More Ksp

  2. Comparing Solubilities The relative solubilities can be deduced by comparing values of Ksp. BUT, BE CAREFUL! These comparisons can only be made for salts having the same ION:ION ratio.

  3. Comparing Solubilities • Which salt is more soluble? • Ag2S Ksp = 1.0 X 10-49 • Ni(CN)2 Ksp = 3.0 X 10-23 • Ag2S  2 Ag+ + S-2Ni(CN)2 Ni+2 + 2 CN- • Since both make 3 ions (4s3) – the larger Ksp is the more soluble salt - Ni(CN)2!

  4. Comparing Solubilities • Which salt is more soluble? • PbCl2 Ksp = 1.6 X 10-5 • PbBr2 Ksp = 4.6 X 10-6 • PbI2 Ksp = 1.4 X 10-8

  5. Comparing Solubilities • Rank the following in order of increasing solubility: • BaF2 Ksp = 1.7 X 10-6 • BaCO3 Ksp = 8.1 X 10-9 • Ag2CO3 Ksp = 8.1 X 10-12

  6. Comparing Solubilities • Rank the following in order of increasing solubility: • BaF2 Ksp = 1.7 X 10-6 s = • BaCO3 Ksp = 8.1 X 10-9 s = • Ag2CO3 Ksp = 8.1 X 10-12 s= BaCO3 Ag2CO3 BaF2

  7. Calculate the effect of a common ion on pH or solubility • Calculate the molar solubility of silver chromate (Ksp = 9.0 X 10-12) in • Water • 0.015 M AgNO3 • 0.015 M K2CrO4

  8. Calculate the effect of a common ion on pH or solubility • Calculate the molar solubility of lead(II) iodide (Ksp = 1.0 X 10-8) in • Water • 0.010 M KI • 0.020 M Pb(NO3)2

  9. Calculate the effect of a common ion on pH or solubility Calculate the solubility of solid CaF2 (Ksp = 4.0 X 10-11) in a 0.025 M NaF solution. Solution = 6.4 X 10-8 mol/L

  10. Determine if a precipitate will form With some knowledge of the reaction quotient (Q), we can decide 1) whether a ppt will form, AND 2) what concentrations of ions are required to begin the ppt. of an insoluble salt.

  11. Determine if a precipitate will form 1. Q = Ksp, the system is at equil. (saturated) 2. Q < Ksp, the system is not at equil. (unsaturated – shift right) 3. Q > Ksp, the system is not at equil. (supersaturated – shift left)

  12. Determine if a precipitate will form Precipitates form when the solution is supersaturated!

  13. Determine if a precipitate will form • Substitute molarities into Q • Compare Q to Ksp • If precipitation occurs, consider the stoichiometry and limiting reactant • Readjust to equilibrium Look at sample 15.16 on P. 766

  14. Determining Precipitation Conditions A solution is prepared by adding 750.0 mL of 4.00 X 10-3M Ce(NO3)3 to 300.0 mL of 2.00 X 10-2M KIO3. Will Ce(IO3)3 (Ksp = 1.9 X 10-10) precipitate from this solution? Yes!

  15. A solution is prepared by mixing 150.0 mL of 1.00 X 10-2 M Mg(NO3)2 and 250.0 mL of 1.00 X 10-1M NaF. Calculate the concentrations of Mg2+ and F- at equilibrium with solid MgF2 (Ksp = 6.4 X 10-9).

  16. Solution [Mg2+] = 2.1 X 10-6M [F-] = 5.50 X 10-2M

  17. Why Would I Ever Care About Ksp ??? Keep reading to find out ! Actually, very useful stuff!

  18. Solubility, Ion Separations, and Qualitative Analysis …introduce you to some basic chemistry of various ions. …illustrate how the principles of chemical equilibria can be applied.

  19. Selective Precipitation A solution of 0.10 M potassium carbonate was added to a mixture of barium and silver ions. Which precipitate will form first? BaCO3 Ksp = 8.1 X 10-9 Ag2CO3 Ksp = 8.1 X 10-12

  20. Separate the following metal ions: silver, lead, cadmium and nickel

  21. From solubility rules, lead and silver chloride will ppt, so add dilute HCl. Nickel and cadmium will stay in solution.

  22. Separate by filtration: Lead chloride will dissolve in HOT water… filter while HOT and those two will be separate.

  23. Cadmium and nickel are more subtle. Use their Ksp’s with sulfide ion. Who ppt’s first???

  24. Precipitation of Insoluble Salts Metal-bearing ores often contain the metal in the form of an insoluble salt, and, to complicate matters, the ores often contain several such metal salts.

  25. Precipitation of Insoluble Salts Dissolve the metal salts to obtain the metal ion, concentrate in some manner, and ppt. selectively only one type of metal ion as an insoluble salt.

  26. Selective Precipitation A solution contains 1.0 X 10-4M Cu+ and 2.0 X 10-3M Pb2+. If a source of I- is added gradually to this solution, will PbI2 (Ksp = 1.4 X 10-8) or CuI (Ksp = 5.3 X 10-12) precipitate first?

  27. Specify the concentration of I- necessary to begin precipitation of each salt.

  28. Solution CuI will precipitate first. Concentration in excess of 5.3 X 10-8M required.

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