**Step 1:** Calculate the freezing point depression of the solution:

$\overline{){\mathbf{\u2206}}{{\mathbf{T}}}_{{\mathbf{f}}}{\mathbf{=}}{\mathbf{\u2206}}{\mathbf{T}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{pure}}{\mathbf{-}}{\mathbf{\u2206}}{\mathbf{T}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{solution}}}$

${\mathbf{\u2206}}{{\mathbf{T}}}_{{\mathbf{f}}}{\mathbf{=}}{\mathbf{0}}{\mathbf{\xb0}}{\mathbf{C}}{\mathbf{-}}(-25\xb0C){\mathbf{=}}$**25°C**

**Step 2:** Calculate the molality of the solution:

$\overline{){\mathbf{\u2206}}{{\mathbf{T}}}_{{\mathbf{f}}}{\mathbf{=}}{{\mathbf{iK}}}_{{\mathbf{f}}}{\mathbf{m}}}$

$\frac{\mathbf{25}\mathbf{\xb0}\mathbf{C}}{\mathbf{\left(}\mathbf{1}\mathbf{\right)}(1.86\frac{\xb0C}{m})}{\mathbf{=}}\frac{\overline{)\left(1\right)(1.86{\displaystyle \frac{\xb0C}{m}})}\left(m\right)}{\overline{)\mathbf{\left(}\mathbf{1}\mathbf{\right)}(1.86\frac{\xb0C}{m})}}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}{\mathit{m}}{\mathbf{=}}\frac{\mathbf{25}\overline{)\mathbf{\xb0}\mathbf{C}}}{\mathbf{\left(}\mathbf{1}\mathbf{\right)}(1.86\frac{\overline{)\xb0C}}{m})}$

What volume of ethylene glycol (C_{2}H_{6}O_{2}), a nonelectrolyte, must be added to 15.0 L water to produce an antifreeze solution with a freezing point of -25.0°C? What is the boiling point of this solution? (The density of ethylene glycol is 1.11 g/cm^{3}, and the density of water is 1.00 g/cm^{3}.)

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Our tutors have indicated that to solve this problem you will need to apply the Freezing Point Depression concept. If you need more Freezing Point Depression practice, you can also practice Freezing Point Depression practice problems.

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Based on our data, we think this problem is relevant for Professor Billman's class at Abilene Christian University.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.