Question One

Question

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 answer should be in units of molarity raised to the appropriate exponent.

Question Two

Would you expect the solubility of PbCl2 in water to change dramatically if it were to be dissolved into a solution of 3.091x10^-4 M KCl?
i)Yes, the solubility of PbCl2 would decrease dramatically.
ii)Yes, the solubility of PbCl2 would increase dramatically.
iii)No, the solubility of PbCl2 would remain roughly unchanged.

Answer 1

..........PbCl2 ==> Pb^2+ + 2Cl^-
Ksp = (Pb^2+)(Cl^-)^2
(Pb^2+) = 4.44g/L, convert to mol Pb^2+ and substitute into Ksp. (Cl^-) will be twice that. Solve for Ksp.
The solubility will decrease dramatically BECAUSE of the common ion effect. You are adding Cl^- from KCl and the solubility equilibrium shown above will be shifted to the left.

Answer 2

Question One
1.7e-5

Question Two (There is a bug in the grader!!! this is the right but the grader mark it as incorrect!!!)

i)Yes, the solubility of PbCl2 would decrease dramatically.

Answer 3

Thank you

Answer 4

Had wrong for question two with I

Answer 5

The density of maple syrup is 1.33g/mL. a bottle of maple Syrup contains 740mL of syrup. What is the mass of maple syrup?

Answer 6

if you want that question answered, post it separately.

Answer 7

No, the solubility of PbCl2 would remain roughly unchanged.

Answer 8

he solubility of PbCl2 would remain roughly unchanged.
right