2006-10-22 18:26:48 · 3 answers · asked by Dastfreadsv 2 in Science & Mathematics ➔ Chemistry
Assume that the solubility is x mole/L
.. .. .. .. .. . MgF2 <=> Mg(+2) + 2F(-)
Dissolve .. .. x
Produce .. .. .. .. .. .. .. .. x .. .. .. 2x
You have a common ion effect so at equilibtium you have
Ksp= [Mg+2][F-]^2= (0.090+x)(2x)^2
I found a value of Ksp=5.16* 10^-11 on the net
It is safe to assume that 0.09>> x and thus 0.090+x=0.09
Thus we simplify the equation to
0.09*4*x^2= 5.16*10^-11=>
x=1.197*10^-5 M= 1.2 * 10^-2 mM
2006-10-23 00:01:43 · answer #1 · answered by bellerophon 6 · 0⤊ 0⤋
first you have to tweak the mainframe then watch out for coagulation. If it Coagulats you will end up with a piece of dreck.
2006-10-23 01:29:23 · answer #2 · answered by Ryan M 2 · 0⤊ 0⤋
I need Ksp for MgF2
.09M*x^2 / MgF2=ksp
solve for x = solubility
MgF2= 1M
Mg = .09M
Ksp = depending
2006-10-23 04:12:34 · answer #3 · answered by bige1236 4 · 0⤊ 1⤋