Option A is correct .
As the reaction is Pbcl2=Pb +2 +2Cl-
Ksp= [Pb+2] [Cl-]2
Which is the correct Ksp expression for PbCl2 (s) dissolving in water? Ksp = [Pb2+] [c1-32...
Which is the correct Ksp expression for Ag2CrO4 (s) dissolving in water? Ksp = [Ag*12(CrO42-1 Ksp = (Ag*12[Cr3+][02-14 Ksp = [A8+][Cro_2-12 Ksp - [Ag*][Cro42-1
For the Dissolving of PbCl2 in water Ksp is 1.7 x 10^-5.
calculate deltaG standard at 25 degrees C.
12. For the dissolving of PbCl2 in water Ksp is 1.7 x 10-5. Calculate AG at 25°C. If [Pb2+] = .010M and [Cl-) = .01M what is AG?
Oc Asp – [Ag2+? [C03-] Which is the correct Ksp expression for Ag2CO3 (s) dissolving in water? Ksp = [Ag2+1 C03-12 O B. Ksp - [Ag2+1 (003-] OA OD . Ksp = [Ag+12 [CO32- Ksp = [Ag"] [CO32-
Consider the dissolution equation of lead(II) chloride. PbCl2 (s) Pb2+ (aq) + 2 C1- (aq) Suppose you add 0.2331 g of PbCl2(s) to 50.0 mL of water. In the resulting saturated solution, you find that the concentration of Pb2+ (aq) is 0.0159 M and the concentration of Cl - (aq) is 0.0318 M. What is the value of the equilibrium constant, Ksp, for the dissolution of PbCl2? Answer:
Consider the equilibrium of PbCl2(s) in water: PbCl2(s) Pb2+(aq) + 2Cl-(aq) What is the effect of adding NaCl(aq) to the equilibrium solution? The sodium ion reduces the Pb2+ to Pb(s). PbCl2 solubility increases due to the common-ion effect. PbNa2(s) precipitates. The NaCl(aq) has no effect on the system. PbCl2(s) precipitates until equilibrium is reestablished.
1. A saturated solution of lead(II) chloride was prepared by dissolving PbCl2 solid in water. The concentration of Pb+2 ion in the solution was found to be 1.62*10^-2M . Calculate Ksp for PbCl2 . 2. The value of Ksp for silver chromate, Ag2CrO4 is 9.0*10^-12 . Calculate the solubility of Ag2CrO4 in grams per liter.
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.
What is the correct expression of the solubility product constant (Ksp) for the following equilibrium? PbCl4 (s) = P64+ (aq) + 4C1- (s) K SP [P0++] [C1-]4 4 [PB+][c1] sp [PbCl4] [Pb++]ax [cr] Ksp = [PbC14] OK sp = [Pb1+] [C1-14
What is the correct expression of the solubility product constant (Ksp) for the following equilibrium? PbC14 (s) = P64+ (aq) + 4Cl- (s) P64+ K 8p [c1"]" Кsp [Pb2+] [c1-14 [PbC14] [Ps+]4x [C] K sp = (PbC14) O Køp = [P64+] [C1-14