The Ksp for PbI2 is 9.8×10−9 . Will PbI2 precipitate if 2.5 mL of 0.0025 M Pb(NO3)2 is added to 7.5 mL of 0.0050 M NaI?
total volume of solution mixture = (2.5 + 7.5) = 10.0 ml
2.5 mL of 0.0025 M Pb(NO3)2 is added to 7.5 mL of 0.0050 M NaI mixed.
[Pb^2+] = [Pb(NO3)2] = 2.5 mL * 0.0025 M / 10.0 ml = 6.25 * 10^-4 M
[I-] = [NaI] = 7.5 mL * 0.0050 M / 10.0 ml = 3.75 * 10^-3 M
PbI2 ............> Pb^2+ + 2 I-
Q = [Pb^2+][I-]^2 = 6.25 * 10^-4 * (3.75 * 10^-3)^2 = 8.79 * 10^-9
we have
Ksp for PbI2 is 9.8×10−9
thus
Q < Ksp
so
PbI2 do not precipitated.
The Ksp for PbI2 is 9.8×10−9 . Will PbI2 precipitate if 2.5 mL of 0.0025 M...
Calculate the number of moles of Pb2+ in 2.5 mL of 0.0025 M Pb(NO3)2 and the number of moles of I – in 7.5 mL of 0.0050 M NaI.
The solubility of PbI2 (Ksp = 9.8 x 10-9) varies with the composition of the solvent in which it was dissolved. In which solvent mixture would PbI2 have the lowest solubility at identical temperatures? a. pure water b. 1.0 M Pb(NO3)2(aq) c. 1.5 M KI(aq) d. 0.8 M MgI2(aq) e. 1.0 M HCl(aq)
If 15.0 mL of 8.80×10-4 M Pb(NO3)2 are added to 22.0 mL of 3.10×10-5 M KI, will solid PbI2 (Ksp = 8.7×10-9) precipitate? If a precipitate will not form, what iodide ion concentration will cause a precipitate of lead iodide to form? If a precipitate will form, what is the minimum [I-] that could have been present without initiating precipitation? Assume the total volume used in the above example. M
If 100.0 mL of 0.0500 F Pb(NO3)2 is mixed with 200.0 mL of 0.100 F NaI will a precipitate of PbI2 from or not? you will need to justify your answer. Ksp(PbI2) = 1.4* 10^-8
What precipitate(s) do you expect from the reaction of Pb(NO3)2 and NaI ? A. PbI2 B. Pb2I and NaNO3 C. NaNO3 D. Pb(NO3)2 E. no precipitate expected
A solution contains 2.2×10−4 M Ag+ and 1.7×10−3 M Pb2+. If NaI is added, will AgI(Ksp=8.3×10−17) or PbI2(Ksp=7.9×10−9) precipitate first? AgI. My question is: Specify the concentration of I− needed to begin precipitation.
23. Will a precipitate form when 100. mL of 8.0x 103 M Pb(NO3)2 is added to 400. mL of 5.0 x 10-3 M Na2SO4? The Ksp of PbSO4 is 6.3 x 10-7 A. No precipitate forms because Qsp Ksp B. Yes, a precipitate forms because Qsp>Ksp C. No precipitate forms because Qsp> Ksp es, a precipitate forms because Qsp Ksp
Calculate the Qsp or Ksp, as indicated, and determine whether a precipitate will form when each of the following mixtures is prepared. (a) 25.12 mL 1.57 ✕ 10−4 M CaCl2 is mixed with 25.13 mL 3.26 ✕ 10−3 M NaF. (Ksp for CaF2 = 3.5 ✕ 10−11) (b) 14.77 mL 3.68 ✕ 10−3M Pb(NO3)2 is mixed with 35.01 mL 1.63 ✕ 10−4M Na2SO4. (Ksp for PbSO4 = 2.5 ✕ 10−8) (c) 50.33 mL 2.62 ✕ 10−2M Pb(NO3)2 is mixed with...
BaCO3 has a Ksp of 1.2×10−10. Is it more or less soluble than PbI2? The Ksp for PbI2 is 9.8×10−9.
Solid PbI2 was added to a 0.030 M NaI solution. Calculate the molar concentration of lead ion in this solution. Ksp = 7.9 x 10-9 (at 25ºC) (Please show work) PbI2(s) <=> Pb2+ + 2I-