Question

How do Intermolecular forces affect solubility?

Answer 1

The strength of the intermolecular forces between matters and solvents determines the solubility of a given solute in a solvent. so for the solution, the matter should be solvated, by the solvent. Solutes with success dissolve into solvents once solute-solvent bonds become stronger than either solute-solute bonds or solvent-solvent bonds.

Complete step by step answer:
There are two theoretic steps to form a solution, each similar to one of the two opposing forces that dictate solubility. If the solute is in a solid or liquid state, it must first be diffuse — So, its molecular units must be pulled apart. It requires energy, and so this step will always work against solution formation (always endothermic, or requires that energy be put into the system).
Polar molecules dissolve in polar solvents (like water) and non-polar molecules can dissolve in non-polar solvents (like hexane).
The type of forces that exist between neighboring molecules are going to be determined by the properties of these molecules.
Polar molecules are going to be drawn to one another by either Hydrogen ($H$) Bonding or dipole-dipole interactions. These intermolecular forces are making this possible by difference in values of electronegativity two atom bonds to one another.
Non-polar molecules are units drawn to one another by forces (like dispersion) and that they don't have dipoles (like $C{H_4}$ ) or they need multiple dipoles that cancel one another out because of their pure mathematics. greenhouse emission is nonionic due to its linear form that produces the molecule nonionic because of the 2 dipoles $O = C = O$ canceling one another out.

Note: We can confirm the solubility of a matter in a solvent by this. In general, solutes whose polarity matches that of the solvent can typically be soluble. As an example, $NaCl$ dissolves simply into water ${H_2}O$ because each of their molecules are polar.