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:
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?