Whate are the equilibrium concentrations of Pb2+ and F- in a saturated solution of lead(II) fluoride if the Ksp of PbF2 is 3.2x10^-8?
[Pb2+] = ______ M
[F-] = _________ M
Whate are the equilibrium concentrations of Pb2+ and F- in a saturated solution of lead(II) fluoride...
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 .
How many moles of lead (II) fluoride, PbF2, can be dissolved in 31.5 L of water? PbF2 (s) + Pb2+ (aq) + 2F (aq) (Ksp = 3.6x10-8) A. 2.1 x 10-3 mol B. 0.083 mol C. 0.019 mol D. 0.066 mol
Learning Goal: To learn how to calculate the solubility from Kspand vice versa. Consider the following equilibrium between a solid salt and its dissolved form (ions) in a saturated solution: CaF2(s)⇌Ca2+(aq)+2F−(aq) At equilibrium, the ion concentrations remain constant because the rate of dissolution of solid CaF2 equals the rate of the ion crystallization. The equilibrium constant for the dissolution reaction is Ksp=[Ca2+][F−]2 Ksp is called the solubility product and can be determined experimentally by measuring thesolubility, which is the amount...
How many moles of lead (II) fluoride, PbF2, can be dissolved in 31.5 L of water? PbF2 (s) -- Pb2+ (aq) + 2F (aq) (Ksp = 3.6x10-8) O A. 0.019 mol OB. 0.066 mol OC.2.1 x 10-3 mol OD. 0.083 mol
1) Use equilibrium ion concentration to calculate Ksp. The Pb2+ concentration in a saturated solution of lead bromide is measured and found to be 1.19×10-2 M. Use this information to calculate a Ksp value for lead bromide. Ksp =___________ 2) Use solubility to calculate Ksp. The solubility of Fe(OH)2 is measured and found to be 1.15×10-3 g/L. Use this information to calculate a Ksp value for iron(II) hydroxide. Ksp =______________
Question 6 (Extra Credit Challenge): When the sparingly soluble salt lead fluoride, PbF2, is added to an acidic solution with [H+] = 1.6 x 10–4 M, the resulting concentration of [Pb2+] after the salt dissolves is determined to be 7.75 x 10–5 M. (a) Determine the equilibrium constant for the dissolving of PbF2 in an acidic solution of H3O+ and (b) given Ka = 6.8 x 10–4, use the value determined in part a to calculate the Ksp for PbF2...
Lead (II) fluoride, PbF2, crystallizes in a cubic unit cell in which the lead ions occupy a face-centered cubic arrangement in the unit cell, and the fluoride ions are located in certain spaces between the lead ions. How many of each ion are contained within a single unit cell? # of Pb2+ ions = ? # of F– ions =?
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.
A saturated solution of lead (II) iodide, PbI2 has an iodide
concentration of 3.0 × 10-3 mol/ L. Calculate the solubility
constant, Ksp, for lead (II) iodide. PbI2 (s) ß---à Pb2+(aq) +
2I-(aq)
A saturated solution of lead (II) iodide, Pbl2 has an iodide concentration of 3.0 x 10-3 mol/ L. Calculate the solubility constant, Ksp, for lead (II) iodide Pbl2 (s) 8 3.5 x 10-8 5.0 x 10-8 2.8 x 10-8 1.4 x 10-8 -à Pb2 (aq)+2I(aq)
precipitate Q=S ox 10-14 3. Determine the concentration of fluoride ion in a saturated solution of PbF2 (in moles/liter), if the Ksp = 3.6 x 10-8 for PbF2