science

In an experiment to determine the solubility of lead chloride (PbCl2), 5.6g of (NH4)2SO4 was added to a
250ml solution containing an unknown amount of dissolved lead chloride (PbCl2) resulting in the formation of
Lead sulfate precipitate. The mass of the lead sulfate precipitate was found to be 1.645g. From the
information provided, calculate the mass of PbCl2 that dissolved in the given volume of solvent (250 ml),
hence the solubility and the solubility product constant (Ksp)

  1. 0
asked by nelo
  1. g PbSO4 = 1.645
    mols PbSO4 = 1.645/molar mass = estimated 0.00542 = estd 0.00542mols Pb = estd 0.00542 mols PbCl2.

    g PbCl2 = mols PbCl2 x molar mass PbCl2 and that is g/250mL. That x 4 = g/L
    Then g/L divided by molar mass PbCl2 = M = (PbCl2) = (Pb^2+).
    (Cl^-) = 2 x (Pb^2+).
    Then Ksp = (Pb^2+)(Cl^-)^2 = ?

    posted by DrBob222
  2. 85g

    posted by Anonymous
  3. 11.676g pbcl2 and ksp= 0.642

    posted by michael

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Question One Lead chloride dissolves in water according to PbCl2(s) Pb^2+ + 2Cl^- (aq) The solubility in pure water has been measured to be 4.44g . L^-1 . Calculate the solubility product of lead chloride in pure water. Your
  2. chem

    the solubility of lead(II) chloride, PbCl2, in water at 20 degrees Celcius is 1.00 g PbCl2/100 g of water. if you stirred 7.50 g PbCl2 in 400 g of water at 20 degrees Celcius, what mass of lead (II) chloride would remain
  3. chemistry

    The solubility of lead (II) chloride (PbCl2) is 1.6 x 10^-2 M. What is the Ksp of PbCl2?
  4. Chemistry

    Lead chloride dissolves in water according to PbCl2(s)↔Pb2++2Cl−(aq) The solubility in pure water has been measured to be 4.44 g⋅L−1. Calculate the solubility product of lead chloride in pure water. Your answer should be
  5. chemistry

    Lead chloride dissolves in water according to PbCl2(s)↔Pb2++2Cl−(aq) The solubility in pure water has been measured to be 4.44 g⋅L−1. Calculate the solubility product of lead chloride in pure water. Your answer should be
  6. chemistry

    Lead chloride dissolves in water according to PbCl2(s)↔Pb2++2Cl−(aq) The solubility in pure water has been measured to be 4.44 g⋅L−1. Calculate the solubility product of lead chloride in pure water. Your answer should be
  7. chemistry

    Use Ksp for PbCl2 and Kf for [PbCl3]− to determine the molar solubility of PbCl2 in 0.10 M HCl(aq). [Hint: What is the total concentration of lead species in solution?]
  8. chemistry

    Would you expect the solubility of PbCl2 in water to change dramatically if it were to be dissolved into a solution of 3.091×10−4 M KCl? Yes, the solubility of PbCl2 would decrease dramatically. Yes, the solubility of PbCl2
  9. science

    A lab technician adds 0.035 mol of KCl to 1.00 L of 0.0050 M Pb(NO3)2. Ksp = 1.7 × 10–5 for PbCl2. Which of the following statements is correct? a) Lead chloride precipitates until the solution is saturated. b) The solution is
  10. Chemistry

    What is the maximum mass(g) of KCL that can be added to 1.00L of a 0.0100 M lead(ii) chloride solution without causing any precipitation of PbCl2? Assume the additional KCl does not affect the volume of the solution. For, PbCl2,

More Similar Questions