The solubility of benzoic acid, is (0.34 mathrm{~g} / 100 mathrm{~mL}) in water at (25^{circ} mathrm{C}) and
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The solubility of benzoic acid,
is \(0.34 \mathrm{~g} / 100 \mathrm{~mL}\) in water at \(25^{\circ} \mathrm{C}\) and \(10.0 \mathrm{~g} / 100 \mathrm{~mL}\) in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}ight)\) at \(25^{\circ} \mathrm{C}\). Rationalize this solubility behavior. For a \(1.0 \mathrm{~m}\) solution of benzoic acid in benzene, would the measured freezing-point depression be equal to, greater than, or less than \(5.12^{\circ} \mathrm{C}\) ? \(\left(K_{\mathrm{f}}=5.12^{\circ} \mathrm{C} \mathrm{kg} / \mathrm{mol}ight.\) for benzene.)
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