Solubility Equilibria

 

The following problems are taken from T. L. Brown, H. E. Lemay, B. E. Bursten, & J. R. Burdge, Chemistry: The Central Science, Ninth Edition, Chapter 17. To see the solution to a problem or to return from the solution, click on the number of the problem.

 

40) A 1.00-L solution saturated at 25°C with lead(II) iodide contains 0.54 g of PbI2. Calculate the solubility product constant for this salt at 25°C.

 

44) Calculate the molar solubility of Fe(OH)2 when buffered at pH:

      (a) 7.0

      (b) 10.0

      (c) 12.0

      

52) (a) Will Co(OH)2 precipitate from solution if the pH of a 0.020 M solution of Co(NO3)2 is adjusted to 8.5?

      (b) Will AgIO3 precipitate when 100 mL of 0.010 M AgNO3 is mixed with 10 mL of 0.015 M NaIO3? (Ksp of AgIO3 is 3.1 x 10-8.)

 


56) A solution of Na2SO4 is added dropwise to a solution that is 0.0150 M in Ba2+ and 0.0150 M in Sr2+.      

      (a) What concentration of SO42- is necessary to begin precipitation?
(Neglect volume changes. Ksp(BaSO4) = 1.1 x 10-10, Ksp(SrSO4) = 3.2 x 10-7.)

      (b) Which cation precipitates first?

      (c)  What is the concentration of SO42- when the second cation begins to precipitate?

 

82) The solubility product constant for barium permanganate, Ba(MnO4)2, is 2.5 x 10-10. Suppose that solid Ba(MnO4)2 is in equilibrium with a solution of KMnO4. What concentration of KMnO4 is required to establish a concentration of 2.0 x 10-8 M for the Ba2+ ion in solution?      


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