1 .		Will Mn(OH)2 precipitate from solution if the pH of a 0.050 M solution of MnCl2 is adjusted to 8.0 (Ksp = 1.8 x 10-11)? Online Text [Hint]
2 .		Would a precipitate be observed if equal volumes of a 0.040 M AgNO3 solution and a 0.030 M NaNO2 solution are mixed (Ksp(AgNO2) = 6.0 x 10-4)? Online Text [Hint]
3 .		Calculate the minimum pH needed to precipitate Ni(OH)2 so completely that the concentration of Ni2+ is less than 1.0 g/L (1.0 part per billion (ppb)) (Ksp = 1.6 x 10-14). Online Text [Hint]
4 .		What pH is needed to precipitate Ni(OH)2 so completely that the nickel concentration is less than 1.1 x 10-5 M (Ksp = 1.6 x 10-14)? Online Text [Hint]
5 .		In which case will a precipitate form? (i) a 0.050 M MnCl2 solution with pH = 8.00 (Does Mn(OH)2 precipitate?) Ksp = 1.9 x 10-13. (ii) 100. mL of 0.010 M AgNO3 is added to 20. mL of .050 M Na2SO4 (Does Ag2SO4 precipitate?) Ksp = 1.4 x 10-5. Online Text [Hint]
6 .		Which would precipitate first upon addition of the sodium salts of the following anions to solutions 0.10 M in Pb(NO3)2?      ion      Ksp of lead salt Online Text [Hint]
7 .		Consider a solution containing 0.181 M lead ions and 0.174 M mercury(II) ions. The Ksp for lead sulfide is 3.4 x 10-28 and that for mercury(II) sulfide is 4.0 x 10-53. Calculate the maximum concentration of sulfide ions that can be in solution without precipitating any lead ions. Online Text [Hint]
8 .		If 0.1 M aqueous solutions of the following pairs of substances are mixed together, which pair could result in the formation of a precipitate? Online Text [Hint]
9 .		In which of the following solutions will a precipitate form? (i) an AgNO3 solution added to a NaCl solution (ii) S2- ions added to a Cu2+ solution (iii) phosphate ions added to a solution containing Mg2+ (iv) Cu2+ added to a solution containing Mg2+ Online Text [Hint]
10 .		When a solution containing an unknown number of metal ions is treated with dilute HCl, no precipitate forms. The pH is adjusted to about 1, and H2S is bubbled through. Again no precipitate forms. The pH of the solution is then adjusted to about 8 and treated with (NH4)2S. This time a precipitate forms. The filtrate from this solution is treated with (NH4)2HPO4. No precipitate forms. Which metal ions discussed in Section 17.7 are possibly present? Online Text [Hint]
11 .		In the course of various qualitative analysis procedures, the following mixture is encountered: Mg2+ and K+. Suggest how this mixture might be separated. Online Text [Hint]
12 .		An aqueous solution containing an unknown metal ion is treated with a chloride solution under acid conditions; however, no precipitate forms. The solution is then treated with a sulfide solution—again under acidic conditions; again, no precipitate appears. When the solution is neutralized with ammonia, however, a precipitate forms. Given a choice of the following metals, which one is most likely to be the unknown metal? Online Text [Hint]
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