Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF. Ksp, BaF2 = 1.7 X 10-6.
Which one of these is the correct answer?
BaF2 molar solubility = 2.3 x 10-5 M
BaF2 molar solubility = 0.0750 M
BaF2 molar solubility = 8.5 x 10-7 M
BaF2 molar solubility = 1.2 x 10-2 M
BaF2 molar solubility = 3.0 x 10-4 M
at equilibrium :
[Ba2+]= x
[F-]= 2x + 0.0750
Ksp = [Ba2+][F-]^2 = (x) ( 2x + 0.0750)^2
x = molar solubility =3.0 x 10^-4 M (answer)
Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF. Ksp, BaF2 = 1.7 X 10-6. Which one of th...
Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF. Ksp (BaF2) = 1.7
Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF. Ksp (BaF2) = 1.7 ? 10^-6. Please do not leave x(2x+.0750)^2 = 3.0x10^-4. I know that is the set up, I know why that is the set up, and I know that, that is the answer. Please show me the work to get that answer. If you have to foil show me the foil method, if you have to add a number, show me. My brain is...
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