[Rutherford]

In an experiment, the solubility of iodine in diethyl ether, n-hexane, carbon  tetrachloride and toluene was measured. The solubilities were: 337g/kg, 182g/kg, 19 g/kg and 13 g/kg. Correlate the solubilities with the solvents.

Iodine has only London dispersion forces present, just as n-hexane and carbon  tetrachloride. Toluene isn't symmetric so there exist a small permanent dipole moment. Diethyl ether should be the most polar. The solutions are: carbon  tetrachloride=19,   n-Hexane=13, Diethyl ether=337, Toluene=182. How so?

[Rutherford]

Any idea?

[Corribus]

This is something of a trick question, because it plays upon your traditional notion of what solubility means.

Here's your bad assumption:

Iodine has only London dispersion forces present

It's not necessarily wrong, but it fails to account for other factors which might influence "solubility" (yes, in quotes). Rather than addressing that directly, I'll ask you a question: have you ever noticed that the color of an iodine solution significantly depends on the solvent? Why might that be.

If you can't come up with a reason on your own, go back over half a century to some of the original work on iodone solutions. Maybe you find your answer in there somewhere.

http://pubs.acs.org/doi/abs/10.1021/ja01158a096

[Rutherford]

Iodine dissolves in iodide. Are you aiming at auto-dissociation of iodine in a solution?

[Rutherford]

The text you attached doesn't explain the process of salvation, how and why does it happen. I need some more info.

[Corribus]

No but it does tell you that certain solvents form charge transfer complexes with iodine, and certain others do not.