Dear Sir. Concerning your issue about how polarity of acetone changes with temperature . Polar molecules tend to arrange themselves head to tail, positive to negative, and these orientations lead to further increases in intermolecular attraction. These dipole-dipole forces, called Keesom interactions, are symmetrical attractions that depend on the same properties in each molecule. Because Keesom interactions are related to molecular arrangements, they are temperature dependent. Higher temperatures cause increased molecular motion and thus a decrease in Keesom interactions. On the other hand, any molecule, even if nonpolar, will be temporarily polarized in the vicinity of a polar molecule, and the induced and permanent dipoles will be mutually attracted. These dipole-induced dipole forces, called Debye interactions, are not as temperature dependant as Keesom interactions because the induced dipole is free to shift and rotate around the nonpolar molecule as the molecules move. Both Debye induction effects and Keesom orientation effects are considered similar in terms of solubility behavior and are collectively referred to as polar interactions or simply polarities. I think the following below link may help you in your analysis:

https://cool.conservation-us.org/coolaic/sg/bpg/annual/v03/bp03-04.html

Thanks

You should describe the influence of temperature on each type of interactions that acetone can exhibit.

regards,

G

I think that the properties of solvents are the ones that determine their uses such as melting point, boiling point and constant electrostatic insulation