PbI2 is a sparingly soluble salt with Ksp= 1.39x10-8 What is the molar solubility of PbI2?
Find the molar solubility of PbI2. Ksp=7.1e-9, then given the molar solubility from the previous answer, what is the solubility of PbI2, in grams per litre? Knowing this, would PbSO4 (Ksp=1.6e-8) have a higher molar solubility than PbI2? (I'm thinking PbSO4 would be higher, since the Ksp is larger?)
The Ksp of PbI2 is 7.9 x 10-9. What is the molar solubility of lead (II) iodide?
1/ The molar solubility of PbI2 is 1.5 x 10-3 M. a/ What is the molar concentration of iodide ion in a saturated PbI2 solution? b/ Determine the solubility constant, Ksp, for lead(II) iodide 2/ Calculate the molar solubility of PBI2 in the presence of 0.10 M NaI 3/ Compare the molar solubility given in problem 1 and the molar solubility calculated in problem 2. Explain the cause of the difference.
6) The molar solubility of PbI2 is 1.5X10-3 mol/L. PbI2(s) ??Pb2+(aq) + 2I-(aq) A) What is the molar concentration of iodide ion in a saturated PbI2 solution? Hint: consider mol ratios. B) Determine the solubility constant, ksp, for lead(II) iodide: ksp = [Pb2+] x [I-]
1) The molar solubility of PbI2 is 1.5X10-3 mol/L. PbI2(s) ? Pb2+(aq) + 2I-(aq) What is the molar concentration of iodide ion in a saturated PbI2 solution in mol/L? Hint: Consider mol ratios. Don't use scientific notation. Use 2 significant figures. ________ 2) The molar solubility of PbI2 is 1.5X10-3 mol/L. PbI2(s) ?Pb2+(aq) + 2I-(aq) Determine the solubility constant, ksp, for lead(II) iodide: ksp = [Pb2+][I-]2 Don't use scientific notation. Use 2 significant figures. ________ 3) How is the molar...
The solubility of PbI2 in water at 20 ˚C is 1.37 x 10-3m. Determine the Ksp in terms of γ+/- Then use the Debye-Hückel limiting law to calculate the Ksp for PbI2. The solubility of PbI2 in water at 20 ˚C is 1.37 x 10-3m. Determine the Ksp in terms of γ+. Then use the Debye-Hückel limiting law to calculate the Ksp for PbI2.
Assuming that no other equilibria other than dissolution is involved, calculate the molar solubility of PbI2 given that the Ksp = 1.4 x 10-8.
1. At 25 deg Celsius, the solubility product constant of PBI2 is 1.4 x 10^-8. Calculate the molar solubility in water. 2. The solubility of AgI at 25 deg Celsius is 9.1 x 10^-4 M. Calculate the Ksp of AgI at that temperature.
If x = molar solubility, Ksp = solubility product, which of the following compounds would have the relationship: 27x4 = Ksp? a) Bi2S3 b) Ag2CO3 c) AgCl d) PbI2 e) Ag3PO4