|Oct20-07, 07:57 PM||#1|
Chemistry- Selective Precipitation
1. The problem statement, all variables and given/known data
My molarity [I] is wrong which keeps me from ding the rest of this problem...any help would be greatly appreciated.
A researcher has a 450.0 mL solution that is 0.421 M in Hg2(NO3)2 and 0.0191 M in Pb(NO3)2. She plans to add solid potassium iodide to separate the mixture by selective precipitation.
Ksp PbI2 = 1.4e-8
Ksp Hg2I2 = 1.2e-28
What is the maximum concentration of iodide ions that may be in solution to achieve the best separation possible?
M [I-]= ?
How many grams of potassium iodide should she add to achieve this?
g of KI
What will the percentage of mercury(I) ions remaining in solution be?
2. Relevant equations
3. The attempt at a solution
hg2i2 = hg2 + 2i
1.2e-28 = [.421][I]^2
[I]= 1.68e^-14, which is wrong and I have no idea what I am doing wrong
|Oct20-07, 11:38 PM||#2|
|Oct21-07, 11:15 AM||#3|
thanks, but I already figured that out
I failed to realize it said MAXIMUM
so [i] would be ksp for pbi
[I] = 8.6e-2
but now I am having problems with b and c
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