What concentration of the lead ion, Pb2+, must be exceeded to precipitate PbCl2 from a solution that is 1.00×10−2 M in the chloride ion, Cl−? Ksp for lead(II) chloride is 1.17×10−5
For precipitate to form minimum condition is,
[Pb+2][Cl-]^2 = Ksp
[Pb+2] [1x10^-2]^2 = 1.17x10^-5
[Pb+2] = 0.117 Moles/litre
What concentration of the lead ion, Pb2+, must be exceeded to precipitate PbCl2 from a solution that is 1.00×10−2 M in...
What concentration of the lead ion, Pb2+, must be exceeded to precipitate PbF2 from a solution that is 1.00×10−2M in the fluoride ion, F−? Ksp for lead(II) fluoride is 3.3×10−8 .
Part A - Calculate the value of Q What is the value of Q when the solution contains 2.00×10?2 M Ca2+ and 3.00×10?2M CrO42?? Express your answer numerically. Part C What concentration of the lead ion, Pb2+, must be exceeded to precipitate PbCl2 from a solution that is 1.00×10?2 M in the chloride ion, Cl?? Ksp for lead(II) chloride is 1.17×10?5 . Express your answer with the appropriate units.
Learning Goal: To understand the relationship between precipitation and the solubility product and to be able to predict whether a substance will precipitate or not. Precipitation is the formation of an insoluble substance. For the equation AB(s)⇌A+(aq)+B−(aq), precipitation represents a shift to the left and the production of a solid. From Le Châtelier's principle, we know that when the product of the concentrations of A+ and B− gets above a certain level, the reaction will respond by shifting left to...
II Review | Constants A solution is 0.070 M in Pb2+. - Part A What minimum concentration of Cl~ is required to begin to precipitate PbCl2 ? For PbCl2, Ksp = 1.17 x 10-5. 0 6.46 x 10-3 M O 9.05 x 10-4 M O 1.29 x 10-2 M O 1.17 x 10-5 M Submit Request Answer
1) For the reaction: PbCl2(s) ↔ Pb2+(aq)+2Cl1-(aq), what is Q* when 2.5 mL of 0.070 M lead nitrate is added to 19 mL of 0.018 M sodium chloride? Ksp of lead chloride is 1.6 x 10-5 M3. Hint given in general feedback *Recall: Q is compared to Ksp to determine whether a precipitate forms. 2) Sodium phosphate is added to a solution that contains 0.0041 M aluminum nitrate and 0.028 M calcium chloride. The concentration of the first ion to...
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:
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 value of Q when the solution contains 2.50×10-3M Mg2+ and 2.00×10-3M CO32-?What concentration of the lead ion, Pb2+ , must be exceeded to precipitate PbF2 from a solution that is 1.00×10-2 M in the fluoride ion, F- Ksp for lead(II) fluoride is 3.3×10-8.
A26. What will be observed when 15.0 mL of 0.040 M lead(II) nitrate, Pb(NO3)2, is mixed with 15.0 mL of 0.040 M sodium chloride? (lead chloride Ksp = 1.7 × 10–5). (A) A clear solution with no precipitate will result. (B) Solid PbCl2 will precipitate and excess Pb2+ ions will remain in solution. (C) Solid PbCl2 will precipitate and excess Cl– ions will remain in solution. (D) Solid PbCl2 will precipitate and there will be no excess ions in solution....
8) Calculate the following for 2.0 L solution containing [Ag+] = 0.100 M and [Pb2+] = 0.100 M. Assume no volume changes. (AgCl Ksp = 1.8 x 10-10, PbCl2 Ksp = 1.8 x 10-5). a) At what [Cl-] will each salt precipitate? b) What percent of the Ag+ has precipitated before the Pb2+ begins to precipitate? c) How much sodium chloride must be added (in grams) to precipitate a maximum AgCl before before any PbCl2 begins to precipitate?