Question
Lead iodide, PbI2, has a Ksp in water of 7.1e-9 M3 at room temperature.
Calculate the solubility of PbI2 in water. Express your answer in grams per liter.
What is the solubility of PbI2 in 0.1 M NaI (aq)? Express your answer in grams per liter.
Calculate the solubility of PbI2 in water. Express your answer in grams per liter.
What is the solubility of PbI2 in 0.1 M NaI (aq)? Express your answer in grams per liter.
Answers
JavaLovesC#
This is simple Stoichiometry problem
Write down PbI2 -> Pb2+ + 2I-
Therefore
Ksp = [Pb2+][I-]^2
From the stoich you can derive that
Ksp = Cs(2Cs)^2 = 4Cs^3
Hence Cs = (Ksp/4) ^ 1/3
Then multiply the Molar Weight to get grams / Liter unit that you like
Write down PbI2 -> Pb2+ + 2I-
Therefore
Ksp = [Pb2+][I-]^2
From the stoich you can derive that
Ksp = Cs(2Cs)^2 = 4Cs^3
Hence Cs = (Ksp/4) ^ 1/3
Then multiply the Molar Weight to get grams / Liter unit that you like
JavaLovesC#
The second problem is common ion effect
First see is the added ion concentration more than or less than your Cs.
0.1 seems to be >>>> than Cs so common ion will happen
Ksp = Cs'(0.1)^2 = 0.01Cs'
Hence
Cs' = Ksp/0.01
Then just multiply by Molar weight again to convert to g/L units .
Note use the Molar Weight of PbI2 !!!!
First see is the added ion concentration more than or less than your Cs.
0.1 seems to be >>>> than Cs so common ion will happen
Ksp = Cs'(0.1)^2 = 0.01Cs'
Hence
Cs' = Ksp/0.01
Then just multiply by Molar weight again to convert to g/L units .
Note use the Molar Weight of PbI2 !!!!