Calculation :
X3Y2 -------> 3X(2+) + 2Y(3-)
given solubility = 4 * 10^-6 mol /L
There is a 3:2 molar ratio between the X3Y2 that dissolves and X2+ that is in solution. In like manner, there is a 3:2 molar ratio between dissolved X3Y2 and Y3- in solution.
Ksp = [X2+]^3[Y3-]^2
Ksp = [4 * 10^-6]^3[4 * 10^-6]^2
Ksp = 1024 * 10^-30
Ksp = 1.02 * 10^-27
Answer
Ksp = 1.02 * 10^-27
4. Determine the Ksp for X3Y2 if its solubility is 4.00 X 106 moles/Litre.
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1)Use the virtual lab to determine the solubility product (Ksp)
for the following solids. Show all work for credit. *should be able
to use the lab to determine the ion concentrations at equilibrium
and use these for the formulas for KSP and then the KSP'S for
solubility. The lab is just to help you get the ion concentration
(a). AgCl (b). SrSO4 (c). Ag2CO3 (d). Sr(IO3)2
2) What is the solubility of the solids listed in question 1, in
moles/liter?...
The molar solubility of a salt is 1.2 x 10-3M. What is its Ksp of this salt in pure water? If 0.005 of a common ion is added to the solution, what is the new solubility (Common ion effect in salts) The solubility of an unknown salt with a formula XY2 is 3.9 x 10-11 mol/L. What is the value of Ksp of this salt?