10 L of a saturated solution of calcium fluoride, CaF2, was evaporated and found to contain 4.28 millimoles (mmol) fluoride. What is the value of Ksp?
CaF2(s) -> <- ca2+ (aq) +2 F- (aq)
How did
Ksp= [Ca2+] [F-]2
become Ksp= [s] [2s]2= 4s3
Cause I thought it was only Ksp= [s] [s]2 = s3
and why 4.28x10-3 have to devide by 10
and why the
[F-] = 4.28 x 10-4 have to eqautes to 2 to have s= 2.14x10-4 M
10 L of a saturated solution of calcium fluoride, CaF2, was evaporated and found to contain...
QUESTION 6 (15 points) A) A saturated solution of calcium fluoride CaF2 is found to contain a concentration of fluoride ions [F] = 3.0 x 10-6 M. What is the value of the solubility product of this salt?
Calcium fluoride, the main component of the mineral fluorite, dissolves to a slight extent in water. CaF2 (s) ⇄ Ca2+ (aq) + 2F-(aq) Ksp = [Ca2+][F-]2 Calculate the Ksp value for CaF2 if the calcium ion concentration has been found to be 2.3×10-4 M.
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