What is the molecular equation for the precipitation reaction that occurs when aqueous solutions of sodium sulfate and lead(II) acetate are mixed?

Will FeS precipitate in a solution that is 0.10 M in Fe(NO3)2, 0.4 M in HCl, and 0.10 M in H2S? Will FeS precipitate if the pH of the solution is adjusted to pH 8 with an NH4+ - NH3 buffer? Kspa = 6 x 10^2 for FeS.

In quantitative analysis, Ag+, Hg2+, and Pb2+ are seperated from other cations by the addition of HCl. Calculate the concentration of Cl-ions required to just begin the precipitation of (a) AgCl, (b) Hg2Cl2, (c) PbCl2 in a solution hav-ing metal-ion concentrations of 0.030 M. What fraction of the Pb2+ remains in solution when the Ag+ just begins to precipitate?

A beaker contains aqueous solutions of calcium and barium nitrates. Aqueous sodium carbonate is added to the beaker, and a precipitate forms. What is the composition of the precipitate?

Determine the minimum concentration of NaF required to cause precipitation of BaF₂ from a 4.0×10⁻² M Ba(NO₃)₂ solution, given that the Ksp of BaF₂ is 1.7×10⁻⁶.

Which of the following represents the molecular equation for the precipitation reaction that occurs when nickel (II) nitrate is mixed with barium sulfide?

Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide: Pb2+(aq) + 2I-(aq) → PbI2(s). Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. If you have 50.0 mL of a 0.100 M Pb(NO3)2 solution, how many milliliters of 3.550 M HI(aq) are needed to completely precipitate the lead ions as PbI2?

Under what condition will a precipitate form in a solution when comparing the ion product (Q) to the solubility product constant (Ksp)?

Suppose that aqueous solutions of barium nitrate and potassium carbonate are mixed. What is the name of the compound that precipitates?