Factors affecting Solubility

Structure

“like dissolves like” DOES NOT SUFFICE AS AN ANSWER ON TEST (SHOCKER!)
Two substances with similar intermolecular forces are likely to be soluble in each other
- Too Generic need to be more specific
Non-polar molecules are soluble in non-polar solvents
- ex. CCl $_{4}$ in C $_{6}$ H $_{6}$ (hydrocarbons are non-polar)
Polar molecules are soluble in polar solvents
- CH $_{3}$ OH in H $_{2}$ O
Ionic compounds are soluble in polar solvents
- NaCl in H $_{2}$ O (ion-dipole interactions)
Why can’t hydrogen bonding mix with something that disperses LDFs
- 3 types of IMFs: Hydrogen (strongest), Dipole-Dipole, LDFs
- In order to break IMFs it requires energy
- Making IMFs it gives out energy
- If we’re breaking hydrogen bonds and making LDF that doesn’t work because net energy isn’t 0 therefore cannot bond

Water - Universal Solvent hydrophilic - polar; tends to dissolve ionic compounds and polar molecules Hydrophobic - non-polar