What is the solubility in gram/liter for CaF2 (Ksp = 3.9 x 10-11)
The salt dissolves as:
CaF2 <----> Ca2+ + 2 F-
s 2s
Ksp = [Ca2+][F-]^2
3.9*10^-11=(s)*(2s)^2
3.9*10^-11= 4(s)^3
s = 2.136*10^-4 M
Molar mass of CaF2 = 1*MM(Ca) + 2*MM(F)
= 1*40.08 + 2*19.0
= 78.08 g/mol
Molar mass of CaF2= 78.08 g/mol
s = 2.136*10^-4 mol/L
To covert it to g/L, multiply it by molar mass
s = 2.136*10^-4 mol/L * 78.08 g/mol
s = 1.67*10^-2 g/L
Answer: 1.67*10^-2 g/L
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