Calcium sulfate, CaSO4, has a Ksp value of 7.10 × 10¬³. What happens when calcium and sulfate solutions are mixed to give 2.00 × 10–³ M Ca²+ and 3.00 x 10-² MSO4²-? A precipitate forms because Q > Ksp. A precipitate forms because Q < Ksp. No precipitate forms because Q > Ksp. No precipitate forms because Q < Ksp.

A solution contains 0.04900 M Ca²+ and 0.09100 M Agt. If solid Na3PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first? When the second cation just starts to precipitate, what percentage of the first cation remains in solution? A solution contains 0.0490 M Ca²+ and 0.0910 M Agt. If solid Na3PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first? O Ca3(PO4)2 Ag3PO4 O Na3PO4 When the second cation just starts to precipitate, what percentage of the first cation remains in solution? percentage: %

A solution containing cobalt (I) ions is added to a solution that is 0.034 M Br– and 0.069 M Cl–. What is the identity of the precipitate that forms, and at what concentration of cobalt (I) ions does this begin to occur? Solubility Product Constants: CoCl  =  2.1 × 10–5 CoBr  =  6.2 × 10–12   No precipitate will form at any concentration of cobalt (I). CoCl,  9.0 × 10–11 M CoBr,  3.0 × 10–4 M CoCl,  6.2 × 10–4 M CoBr,  1.8 × 10–10 M

A student mixes 33.0 mL of 2.94 M Pb(NO,),(aq) with 20.0 mL of 0.00217 M Na, SO,(aq). How many moles of PbSO,(s) precipitate from the resulting solution? The Ksp of PbSO,(s) is 2.5 × 10-8. 4 4 PBSO, (s) = 4.34 x10-5 m What are the values of [Pb2+], [SO], [NO,], and [Na+] after the solution has reached equilibrium at 25 °C? [Pb2+] = [NO,] = I [So;"] = [Na*] = ?