Final answer:
Sodium benzoate interacts with water primarily through hydrogen bonding, due to its carboxylate group. While its ionic nature suggests possible ionic bonding with water, this interaction is actually characterized as ion-dipole interactions. Sodium benzoate's aromatic ring decreases its overall polarity and solubility compared to fully ionic compounds.
Step-by-step explanation:
The strongest intermolecular force with which sodium benzoate will interact with the solvent water is hydrogen bonding. Sodium benzoate is structurally similar to benzoic acid, consisting of a benzoate ion (the conjugate base of benzoic acid) and a sodium ion. Due to the presence of the carboxylate group, the benzoate ion can form hydrogen bonds with water molecules. Although it is an ionic compound and could potentially form ionic bonds with water, the complete solvation of the ions by water molecules is better defined as ion-dipole interactions. Hydrogen bonds are strong intermolecular interactions, stronger than dipole-dipole interactions and London dispersion forces, which leads to a decent solubility in water. However, it is important to note that the nonpolar aromatic ring also present in sodium benzoate reduces its overall polarity, making its solubility less than that of a fully ionic compound like LiCl but more than that of a completely nonpolar compound like naphthalene.