Which member of each of the following pairs would you expect...

Which member of each of the following pairs would you expect to be more soluble in water? Briefly explain your choices.
a. 2,3-pentanediol or 2,3,4-pentanetriol
b. Hexane or 3-hexanol
c. 1-butanol or 2-octanol

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Key Concepts

Hydrogen Bonding

Hydrogen bonding is a strong type of dipole-dipole interaction that forms when a hydrogen atom covalently bound to an electronegative atom (like oxygen) interacts with another electronegative atom that has a lone pair of electrons. This interaction is key in water solubility because molecules capable of forming hydrogen bonds with water are more easily solvated.

Polarity

Polarity refers to the presence of a distribution of electrical charge over the atoms joined by the bond. In molecules, regions with partial charges interact favorably with the polar water molecules, enhancing solubility. Molecules with polar functional groups are more likely to dissolve in water due to these electrostatic attractions.

Molecular Structure and Hydrophobic-Hydrophilic Balance

The overall water solubility of a compound is determined by the balance between its hydrophilic (water-attracting) parts, such as hydroxyl groups, and its hydrophobic (water-repelling) parts, such as hydrocarbon chains. A compound with more hydrophilic groups or a shorter hydrophobic chain will generally have greater water solubility.

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