Final answer:
CH3Br is expected to be more soluble in water than CBr4 because it is partially polar and can interact with water molecules, whereas CBr4 is nonpolar and cannot.
Step-by-step explanation:
Between CBr4 and CH3Br, CH3Br would be expected to be more soluble in water. Solubility in water is facilitated by the ability to form hydrogen bonds or engage in dipole-dipole interactions with water molecules. CH3Br, being partially polar due to the presence of C-H and Br-H bonds, is capable of interacting with the polar water molecules more effectively than CBr4, which is nonpolar due to its symmetry. On the other hand, CBr4 lacks any polar C-H bonds and thus has limited solubility in water due to its inability to form significant interactions with the polar water molecules.