13. Solubility Problems

  1. The solubility of silver bromide in pure water is measured to be 8.4μg of AgBr per 100. mL of water.  From this data, calculate the solubility in mol/L and the solubility product constant of AgBr.                                      [4.5×10-7 M, 2.0×10-13]
  2. Calculate the solubility of BaSO4 in pure water from solubility product data (Appendix 7)         [1.0×10-5 M]
  3. Calculate the solubility of PbSO4 in pure water from solubility data.                                                  [1.6×10-4 M]
  4. Calculate the solubility of Hg2Cl2 in pure water from solubility data.                                                   [1.0×10-3 M]
  5. Calculate the solubility in pure water of CaC2O4·H2O from solubility data.
    Give the results in mol/L and in g/L                                                                                                              [4.8×10-5 M, 7.0×10-3 g/mol]
  6. What mass of lead bromide, PbBr2 , can be dissolved in 150 mL of pure water?                          [0.66 g]
  7. What is the solubility of BaSO4 in a solution of 0.10 M Na2SO4?                                                         [1.1×10-9 M]
  8. A solution contains cupric ions (Cu2+), manganese ions (Mn2+) and zinc ions (Zn2+) in approximately equal concentrations. The solution is made basic and sodium sulfide is added, which will precipitate all three metal ions as sulfides.  A solution of sulfuric acid is added slowly, thus decreasing the pH.  Which of the precipitates dissolves first, which is second and which is the last to dissolve?                                                                                            [MnS, ZnS, CuS]
  9. If you have a container with the solid mineral galena (PbS) in contact with a buffer solution at pH=6, what is the concentration of the lead.                                                                                                                          [5×10-10 M]
  10. Calculate the solubility of silver bromide, AgBr, in a solution containing ammonia at a concentration of 0.080 M.  The equilibrium constant for the equilibrium below is Kcx2= 1.7×107.                                                                   [2.4×10-4 M]
    Ag+(aq) + 2 Cl–(aq) \rightleftarrows AgCl2–(aq)
  11. Calculate the solubility of silver chloride in a solution tontaining codium chloride, NaCl, at a concentration of 0.080 M. The equilibrium constant for the equation
    Ag+(aq) + 2Cl–(aq) \rightleftarrowsAgCl2–(aq)             is Kcx2= 1.8×105.                                              [2.5×10-5 M]

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