Question
Use a phase diagram to show the difference in freezing points and boiling points between an aqueous urea solution and pure water.
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Calculate the freezing and boiling points (at $760 \mathrm{mmHg}$ ) of a solution of $4.00 \mathrm{~g}$ urea $, \mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2},$ dissolved in $75.0 \mathrm{~g}$ water.
A solution contains $2.00 \mathrm{~g}$ of the nonvolatile solute urea (molar mass $=60.06 \mathrm{~g} / \mathrm{mol}$ ) dissolved in $25.0 \mathrm{~g}$ water. Using the data in Table 12.4 , calculate the freezing and boiling points of the solution in degrees Celsius.
A solution of urea (mol. mass $56 \mathrm{~g} \mathrm{~mol}^{-\mathrm{t}}$ ) boils at $100.18^{\circ} \mathrm{C}$ at atmospheric pressure. If $\mathrm{K}_{\mathrm{f}}$ and $\mathrm{K}_{b}$ for water are $1.86$ and $0.512 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$ respectively, the above solution will freeze at (a) $6.54^{\circ} \mathrm{C}$ (b) $-6.54^{\circ} \mathrm{C}$ (c) $-0.654^{\circ} \mathrm{C}$ (d) $0.654^{\circ} \mathrm{C}$
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