For the Dissolving of PbCl2 in water Ksp is 1.7 x 10^-5. calculate deltaG standard at...
Which is the correct Ksp expression for PbCl2 (s) dissolving in water? Ksp = [Pb2+] [c1-32 Ksp = [Pb2+] [61] Ksp = [Pb2+12 [014] Ksp = [PbCit] [C1) Ksp = [Pb+] (C12-2
For PbCl2, the Ksp = 1.7 x 10-5. What is the solubility of PbCl 2 in 1.0 M NaCl? O a. 4.1 x 10-3 M O b. 2.6 x 10-2 M O c. 1.6 x 10-2 M O d. 1.7 x 10-4 M O e. 1.7 x 10-5 M
Calculate the molar solubility of PbCl2 in a 0.20 M NaCl solution. The Ksp of PbCl2 = 1.7 x 10^–5. (hint: can any assumptions be made to simplify thiscalculation?)A. 4.1 x 10^–3 MB. 4.3 x 10^–4 MC. 8.5 x 10^–5 MD. 3.6 x 10^–6 ME. 1.6 x 10^–2 M
Calculate the solubility of lead chloride, PbCl2 in units of grams per liter. Ksp(PbCl2) = 1.7×10-5. solubility = g/L
Ksp of PbCl2(s) = 1.7x10-5 Delta Gf of PbCl2 = -314KJ/mol Delta Gf of Pb2+ = -24.3KJ/mol Calculate the standard free energy change for the formation of Cl-
Chapter 15 Question 9 1)A saturated solution of lead(II) chloride, PbCl2, was prepared by dissolving solid PbCl2 in water. The concentration of Pb2+ ion in the solution was found to be 1.62×10−2 M . Calculate Ksp for PbCl2. 2)The value of Ksp for silver sulfate, Ag2SO4, is 1.20×10−5. Calculate the solubility of Ag2SO4 in grams per liter.
Ksp of AgCl = 1.77x10^-10 Ksp of PbCl2 = 1.70x10^-5 thanks! A solution contains 0.036 M Ag+ and 0.032 M Pb2+. If you add CI", AgCl and PbCI, will begin to precipitate. What is the concentration of Cl" required, in molarity, when AgCl precipitation begins? concentration of Cl" = What is the concentration of Cl required, in molarity when AgCl precipitation is 99.99% complete? concentration of Cl" = What is the concentration of CI required, in molarity when PbCl, precipitation...
A galvanic cell Pb│PbCl2│NaCl (0.0100M)││AgNO3 (0.500 M)│Ag is setup in the lab. Ksp PbCl2 = 87× 10-5. What is the concentration of Pb2+ in the Pb│PbCl2 half-cell? (10 pts.) Calculate Ecell. (20 pts.) E0 red=-0.13 Pb2+ + 2e- --> Pb E0 red= 0.80 Ag+ + e= -->Ag
The solubility of PbCl2 in a .10M NaCl solution is 1.7*10^-3 mol/L at 25 degrees C. Calculate Ksp for PbCl2. (Note this is a "common ion effect" problem.) Please show all work!
What is the Molar Solubility (concentration, M) of PbCl2 in pure water. Remember that its Ksp = 1.17 X 10-5. PbCl2 (aq) = Pb2+ (aq) + 2Cl- (aq) 1.43 X 10-2M 1.21 X 102 M O 7.19 X 10-5M O 1.50 M