# SOLUBILITY_PROBLEMS

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```					                      SOLUBILITY or Ksp PROBLEMS!

1. Write the general solubility product constant expressions for the
following salts:

a. PbCrO4          b. Fe(OH)3             c. AgI         d. Zn(OH)2
e. Mg3(PO4)2

2. Barium sulfate is a compound that is used to highlight X-rays to identify
cancerous growths. Because it is not very soluble in water, it does not dissolve
well in the GI tract, and enhances the energy of the x-ray. What is the solubility
of each ion in solution? The Ksp for barium sulfate is 1.1 x 10-10.
3. Calculate the Ksp value for bismuth sulfide, which has a solubility of 1.0 x 10-15
mol/L for each ion at 250C.
4. The Ksp for barium iodate at 250C is 6.0 x 10-10. What is the molar solubility of
each ion at 250C in solution? Barium iodate is used to purify edible oils.
5. The Ksp for copper (II) iodate is 1.4 x 10-7 at 250C. Calculate the solubility of
each ion at 250C.
6. The Ksp for La(OH)3 at 250C is 1 x 10-19. Calculate the concentration of each ion
in solution at equilibrium. La(OH)3 is used in solid form in movie lighting and
projection.
7. By experiment, it is found that 1.2 x 10-3 mol of lead iodide dissolves in 1 liter of
aqueous solution at 250C. What is the Ksp at this temperature?
8. The mineral fluorite is calcium fluoride. Calculate the solubility in moles per liter
(M) of each ion of calcium fluoride in water from the solubility product constant,
which is 3.4 x 10-11.
9. Iron (III) hydroxide is used to remove deadly arsenic from drinking water.
Calculate the equilibrium concentrations of each ion in solution.
10. Strontium phosphate is used in the manufacture of fluorescent lights. What is the
solubility of each ion in solution at equilibrium?
11. Silver carbonate is a commonly used pesticide in California. If the silver ion
concentration at equilibrium is 1.27 x 10-4M, calculate the Ksp for silver
carbonate.
12. Copper (I) bromide has a measured solubility of 2.0 x 10-4 mol/L at 250C. This is
how much of each ion dissolves at 250C. Calculate its Ksp value.
13. The concentration of calcium ion in blood plasma is .0025M. If the concentration
of oxalate ions is 1.0 x 10-7M, do you expect calcium oxalate, which is a main
component of kidney stones, to precipitate? The Ksp for calcium oxalate is 2.3 x
10-9.
14. What is the molar solubility of calcium oxalate solid in .15M calcium chloride
solution? Compare this molar solubility to that for calcium oxalate in pure water,
which is 4.8 x 10-5. The Ksp for calcium oxalate is 2.3 x 10-9.
15. What is the solubility of silver ion and chloride ion in a .040 M solution of NaCl
at 250C?
16. The Ksp of mercurous bromide is 1.3 x 10-21 at 250C. Calculate the concentration
of mercurous ion and bromide ion in a .034M solution of KBr at 250C.
17. The solubility product constant of calcium sulfate is 2.4 x 10-5 at 250C. Calculate
the molar solubility of calcium sulfate in a .008M solution of CaCl2 at 250C.
18. What are the equilibrium concentrations of the silver and chromate ion in a
solution that contains silver chromate and .1M silver nitrate? Compare these
values to the equilibrium concentrations of ions of silver chromate in pure water,
which is 1.3 x 10-4 mol/L.
19. Calculate the solubility of solid calcium fluoride in a .025 M sodium fluoride
solution. The Ksp for CaF2 is 4.0 x 10-11.
20. Calculate the solubility of solid calcium fluoride in a .010M Ca(NO3)2 solution.
21. A solution is prepared by adding 750 mL of a 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?
22. What are the equilibrium concentrations of Pb+2 and I-1 ions in a solution formed
by mixing 100 mL of .05M lead (II) nitrate and 200 mL of .1M NaI? Will solid
lead (II) iodide form? The Ksp for PbI2 is 1.4 x 10-8.
23. A solution contains 1.0 x 10-4M Cu+1 and 2.0 x 10-3M Pb+2. If a source of I-1 is
added gradually to this solution, will PbI2 or CuI precipitate first? Specify the
concentration of I-1 necessary to begin precipitation of each salt. The Ksp for CuI
is 5.0 x 10-12.
24. Will a precipitate form when .010L of 8.0 x 10-3M Pb(NO3)2 is added to .40 L of
5.0 x 10-3M Na2SO4? The Ksp for PbSO4 is 1.3 x 10-8.
25. A solution contains 1.0 x 10-2M Ag+1 and 2.0 x 10-2M Pb+2. When Cl-1 is added
to the solution, AgCl (Ksp = 1.8 x 10-10) and PbCl2 (1.7 x 10-5) precipitate from the
solution. What concentration of Cl-1 is necessary to begin the precipitation of
each salt? Which salt precipitates first?

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