SOLUBILITY or Ksp PROBLEMS!
YOU WILL NEED A CHART OF Ksp VALUES
TO COMPLETE SOME OF THESE PROBLEMS
1. Write the general solubility product constant expressions for the
following salts:
a. PbCrO4
e. Mg3(PO4)2
b. Fe(OH)3
c. AgI
d. Zn(OH)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 molar
solubility of each ion in solution? The Ksp for barium sulfate is 1.10 x 10-10.
3. The Ksp for copper (II) carbonate is 2.50 x 10-10 at 250C. Calculate the molar
solubility of each ion at 250C.
4. Calculate the Ksp value for bismuth sulfide, which has a molar solubility for Bi+3
of 3.00 x 10-15 mol/L, and a molar solubility for S-2 of 2.00 x 10-15 mol/L at 250C.
5. The Ksp for barium iodate at 250C is 6.00 x 10-10. What is the molar solubility of
each ion at 250C in solution? Barium iodate is used to purify edible oils.
6. The Ksp for La(OH)3 at 250C is 1.00 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 the molar solubility of Pb+2 is 1.20 x 10-3 M when
lead (II) iodide attempts to dissolve in 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 molar solubility of silver ion in a .040 M solution of NaCl at 250C, if
AgCl solid is attempting to dissolve?
16. The Ksp of silver carbonate is 8.1 x 10-12 at 250C. Calculate the concentration of
carbonate ion that could dissolve into a .034M solution of silver nitrate and solid
silver carbonate 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 .0080M 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 .10M silver nitrate? Compare these
values to the molar solubility of silver chromate in pure water, which is 1.3 x 10-4
mol/L.
19. Calculate the molar 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 molar solubility of solid calcium fluoride in a .010M Ca(NO3)2
solution.