What happens to freezing point of benzene when small quantity of napthalene is added to benzene?

<p>When a small quantity of naphthalene is added to benzene, the freezing point of benzene decreases. This phenomenon is due to the colligative property known as freezing point depression. The addition of a solute, such as naphthalene, disrupts the orderly arrangement of solvent molecules in the solid phase, thereby lowering the freezing point.</p> <p>Mathematically, the decrease in freezing point ($\Delta T_f$) can be represented by the equation:</p> <p>$\Delta T_f = i \cdot K_f \cdot m$</p> <p>where:</p> <p><p>$i$ is the van't Hoff factor (which is 1 for naphthalene as it does not dissociate in solution),</p></p> <p><p>$K_f$ is the cryoscopic constant of the solvent (benzene),</p></p> <p><p>$m$ is the molality of the solution.</p></p> <p>Thus, the correct option is:</p> <p><strong>Option B: Decreases</strong></p>