Solubility Equilibrium – Practice
Name:________________________
1) Write the balanced equation and solubility product expressions for the following solubility
equilibria for the following compounds.
a) Ag2CrO4
b) AuCl3
2) Calculate the concentration of ions in the following saturated solutions:
a) [I-] in AgI solution with [Ag+] = 9.1 x 10-9 M. (Ksp : 8.3 x 10-17)
b) [Al3+] in Al(OH)3 solution with [OH-] = 2.9 x 10-9 M. (Ksp : 1.8 x 10-33)
3) Calculate the solubility products (Ksp) for the following compounds:
a) SrF2 7.3 x 10-2 g/L
b) Ag3PO4 6.7 x 10-3 g/L
4) The molar solubility of MnCO3 is 4.2 x 10-6 M. What is the Ksp for this compound?
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5) The solubility of an ionic compound MX (mol mass = 346 g/mol) is 4.63 x 10-3 g/L. What is
the Ksp for this compound?
6) What is the pH of a saturated zinc hydroxide solution? (Ksp : 1.34 x 10-14)
7) The solubility product of PbBr2 is 8.9 x 10-6. Determine the molar solubility in:
a) pure water,
b) 0.20 M KBr
c) 0.20 M Pb(NO3)2.
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8) If 20.0 mL of 0.10 M Ba(NO3)2 is added to 50.0 mL of 0.10 M Na2CO3, will BaCO3
precipitate? (Ksp : 8.1 x 10-9)
9) Which of the following ionic compounds will be more soluble in acid solution than pure
water:
a) BaSO4
b) PbCl2
c) Fe(OH)3
d) CaCO3.
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