Which solvent, water or hexane \(\left(\mathrm{C}_{6} \mathrm{H}_{14}\right),\) would you choose to dissolve each of the following? a. \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\) b. \(\mathrm{CS}_{2}\) c. \(\mathrm{CH}_{3} \mathrm{OH}\) d. $\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{16} \mathrm{CH}_{2} \mathrm{OH}$ e. \(\mathrm{HCl}\) f. \(\mathrm{C}_{6} \mathrm{H}_{6}\)

. To decide the best solvent for each substance, first, we need to determine whether each substance is polar or non-polar. a. Cu(NO₃)₂: This is an ionic compound, as it has a metal (Cu) and a polyatomic ion (NO₃⁻). Ionic compounds are polar. b. CS₂: This molecule has a linear shape and has no polar bonds, making it a non-polar molecule. c. CH₃OH: Methanol contains a polar O-H bond and has a polar molecular geometry, making it a polar molecule. d. CH₃(CH₂)₁₆CH₂OH: This compound is a long-chain alcohol, primarily non-polar due to the long hydrocarbon chain, but with a polar O-H bond at the end. e. HCl: HCl is a simple covalent molecular compound with a polar bond, making it a polar molecule. f. C₆H₆: Benzene contains non-polar C-C and C-H bonds, and has a symmetric molecular geometry, making it a non-polar molecule.

. Now that we have determined the polarity of each substance, we can choose the best solvent for each one based on the "like dissolves like" concept. a. Cu(NO₃)₂: As an ionic compound (polar), it would dissolve better in water, a polar solvent. b. CS₂: Being a non-polar molecule, it would dissolve better in hexane, a non-polar solvent. c. CH₃OH: This polar molecule would dissolve better in water, a polar solvent. d. CH₃(CH₂)₁₆CH₂OH: This compound has both polar and non-polar regions. Due to the majority of the molecule being non-polar, it would dissolve better in hexane, a non-polar solvent. e. HCl: HCl is a polar molecule, so it would dissolve better in water, a polar solvent. f. C₆H₆: As a non-polar molecule, benzene would dissolve better in hexane, a non-polar solvent.