posted by qwerty on .
Which of the following solution has greater density?
1. 100ml of saturated aqueous solution of Lif. (Ksp(Lif)=1.84*10^-3).
2. 100ml of saturated aqueous solution of Hg2F2. (Ksp(Hg2F2)=3*10^-6).
(We can assume that adding the dissolved doesn't change the volume of the solution).
Explanation would be appreciated.
Use the Ksp values for LiF and Hg2F2 to calculate the solubility of each salt in 100 mL H2O. Then, since density = mass/volume, and the volume is the same, the one with the larger mass will have the largaer density.
So please tell what am I doing wrong here.
As far as I understand the concentration of Lif is the square root of it's ksp=sqrt(1.84*10^-3)=0.043.
Now, 0.043=n/100ml, and by multiplying both sides of the equation by 25.941 (the Mw of Lif) I get that the solubility of Lif in 100ml of water is 1.12g/100ml (which according to wikipedia is wrond...).