In this set of practice problems, we will work on calculating the solubility product constant (Ksp) from the molar solubility of the compound, and vice versa, the Ksp of compounds in pure water, in the presence of salts with common ions, and when the pH of the solution is changed.
1.
Write balanced equations for the dissolution reactions and solubility product expressions for the following compounds.
a. Ca(OH)2 b. Al(OH)3 c. Ba3(PO4)2 d. Pb(IO3)2 e. FeCO3 f. Ag2S
a)
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b)
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c)
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d)
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e)
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f)
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2.
Calculate the Ksp for calcium oxalate, CaC2O4 given its solubility in water is 4.8 x 10-5 mol/L.
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3.
Calculate the Ksp for silver sulfate, Ag2SO4 given its solubility in water is 0.0162 mol/L.
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4.
Determine the Ksp for calcium hydroxide, Ca(OH)2 if its saturated solution has a pH of 12.35.
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5.
Calculate the concentration of phosphate ions in a saturated solution of Ca3(PO4)2 given that Ksp for Ca3(PO4)2 is 1.3 x 10-32 mol/L.
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6.
The Ksp for Hg2Cl2 is 1.1 x 10-18. Calculate the molar solubility of Hg2Cl2 at 20 oC.
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7.
The concentration of Cl– ions in a solution saturated with PbCl2(s) is 0.0318 M. Calculate Ksp for PbCl2.
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8.
Calculate the solubility of silver phosphate, Ag3PO4 in grams per liter of water, given that Ksp is 1.8 x 10-18. Ignore any acid–base properties of the ions.
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9.
The Ksp for chromium (III) hydroxide, Cr(OH)3 is 6.7 x 10-31. Calculate the solubility of Cr(OH)3 in g/L of water.
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10.
Calculate the molar solubility of Al(OH)3 (Ksp = 2.0 x 10-32) in each of the following solutions.
a) Pure water
b) a solution buffered at pH = 6.0
c) a solution buffered at pH = 10.0
a)
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b)
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c)
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11.
The Ksp for silver chromate (Ag2CrO4) is 9.0 x 10-12. Calculate the solubility of silver chromate in each of the following solutions.
a) Pure water
b) 0.15 M AgNO3
c) 0.20 M Na2CrO4
a)
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b)
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c)
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12.
Calculate the solubility of solid Ba3(PO4)2 (Ksp = 6.0 x 10-39) in a 0.10 M K3PO4 solution.
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13.
The Ksp for zinc hydroxide, Zn(OH)2 is 4.5 x 10-17. Determine the pH of a saturated solution of zinc hydroxide.
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14.
If 30.0 mL of 0.10 M Ba(NO3)2 are added to 50.0 mL of 0.10 M Na2SO4, will there be any precipitation observed? Ksp for BaSO4 is 1.5 × 10−9
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15.
Will a precipitate form when 200. mL of 0.035 M Pb(NO3)2 is added to 200. mL of 0.065 M NaCl? Ksp for PbCl2 is 1.6 × 10−5.
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