Lecture 04, concept 05: The hydrophobic effect

[@oscezrcd]

The argument regarding solubility vs. temperature is not correct. Dissolving oil makes entropy decrease, but that alone does not tell you the solubility-temperature dependence. G=H-TS=-kTln(solubility), from this, one can derive kln(solubility)=S-H/T. So d(solubility)/dT is actually controlled by the sign of H, not S.

[@phillipthomas2249]

I was confused by that too. Isn’t the overall delta G what really matters regarding the direction of reaction? So if T goes up your entropy can be lower and still have the same delta G as a reaction with lower temp and higher entropy. It sounds like hydrophobic effect is tied to entropy as the driving factor,so if you raise temperature the drive from entropy would seem to matter less right? Because you wouldn’t need it to result in a negative delta G..?