Which of the following aqueous solutions will have the highest freezing point? A). 1.0 M KCl B). 1.0 M Na$_2$SO$_4$ C). 1.0 M Glucose D). 1.0 M AlCl$_3$

The correct answer is 1.0 M Glucose. The freezing point depression is $\Delta T_f = i \cdot K_f \cdot m$. **Higher $i$ → greater depression → lower freezing point.** | Solute | Dissociation | $i$ | $\Delta T_f$ | |---|---|---|---| | KCl | K$^+$ + Cl$^-$ | 2 | $2K_f$ | | Na$_2$SO$_4$ | 2Na$^+$ + SO$_4^{2-}$ | 3 | $3K_f$ | | **Glucose** | No dissociation | **1** | $K_f$ | | AlCl$_3$ | Al$^{3+}$ + 3Cl$^-$ | 4 | $4K_f$ | **Glucose** has $i = 1$ (non-electrolyte) — the **smallest** depression → **highest freezing point**. AlCl$_3$ has the greatest depression → lowest freezing point.

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