A student measures the molar solubility of magnesium
fluoride in a water solution to be
1.19×10-3 M.
Based on her data, the solubility product constant for this
compound is__________
At equilibrium:
MgF2 <----> Mg2+ + 2 F-
s 2s
Ksp = [Mg2+][F-]^2
Ksp = (s)*(2s)^2
Ksp = 4(s)^3
Ksp = 4(1.19*10^-3)^3
Ksp = 6.741*10^-9
Answer: 6.74*10^-9
A student measures the molar solubility of magnesium fluoride in a water solution to be 1.19×10-3...
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