For each of the following molecules, would you expect greater solubility in water or in hexane? Consider ${\mathrm{CH}}_3\mathrm{OH}$ (methanol).

• A. Insoluble in both water and hexane.
• B. Greater solubility in water due to hydrogen bonding.
• C. Greater solubility in hexane due to its nonpolar nature.
• D. Equally soluble in both solvents.

Answer: (B)

Verified step by step guidance

1. Identify the polarity of the molecule in question. Methanol (CH\_3OH) contains a polar hydroxyl (OH) group capable of hydrogen bonding, making it polar overall.
2. Recall the principle 'like dissolves like,' meaning polar molecules tend to dissolve better in polar solvents, and nonpolar molecules dissolve better in nonpolar solvents.
3. Recognize that water is a highly polar solvent capable of hydrogen bonding, while hexane is a nonpolar solvent.
4. Since methanol can form hydrogen bonds with water molecules, it will have greater solubility in water compared to hexane.
5. Conclude that the presence of the polar OH group in methanol leads to stronger interactions with water, resulting in greater solubility in water than in hexane.