Which, if any of the following mixtures will result in a precipitate.  You might need to know that the Ksp for AgCN is 2.2 x 10-16 and that for PbI2 is 7.9 x 10-9. I.  a mixture that is 1.2 x 10-6 M AgNO3 and 2.4 x 10-10 M NaCN II.  a mixture that is 2.3 x 10-4 M Pb(ClO4)2 and 4.6 x 10-3 M KI

Will a precipitate form when 1.5 mL of 4.5 × 10-3 M ammonium bromate is added to 120.5 mL of 2.5 × 10-3 M silver nitrate? (Ksp for silver bromate is 5.3 x 10-5)

9. Calculate the molar solubility of aluminum hydroxide, Al(OH)3, in a 0.015-M solution of aluminum nitrate, AI(NO3)3. The Ksp of Al(OH)3 is 2x10-32. 1

16. For PbCl2 (Ksp = 2.4 x 10), will a precipitate of PbCl2 form when 100 mL of 3.0 x 10-2 M Pb(NO3)2 is added to 400 mL of 9.0 x 10-2 M NaCl? a) No, because Q = Ksp b) Yes, because Q > Ksp No because K d) No, because Q > Ksp e) Yes, because Q

Will a precipitate form when 20.0 mL of 1.8 x 10-3 M Pb(NO3)2 is added to 30.0 mL of 5.0 x 10-4 M Na2SO4? The Ksp of PbSO4 is 6.3x10-7. A) No because the ion product, Q<Ksp B) No because the Ksp equals the ion product C) No because the ion product, Q>Ksp D) Yes because the ion product, Q>Ksp E) Yes because the ion product, Q<Ksp

Calculate the molar solubility of TZ₂ in a solution that is 0.25 M JoZ. Ksp TZ₂= 5.16 X 10-11. Note: TZ₂ is a nonexistent, ionic compound. 2.35 X 10 -5 2.9 X 10 -5 8.3 X 10 -10 O 2.1 X 10-10

If 12.0 mL of 1.33x104 M AgCH3COO are added to 12.0 mL of 4.50x105 M NaOH, will solid AgOH (Ksp = 2.0x10-8) precipitate? If a precipitate will not form, what hydroxide ion concentration will cause a precipitate of silver hydroxide to form? If a precipitate will form, what is the minimum [OH] that could have been present without initiating precipitation? Assume the total volume used in the above example. M