Problem: What volume of ethylene glycol (C2H6O2), 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/cm3, and the density of water is 1.00 g/cm3.)

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

FREE Expert Solution

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

Tf=T°f,pure-T°f,solution


Tf=0°C-(-25°C)=25°C

Step 2: Calculate the molality of the solution:

Tf=iKfm

25°C(1)(1.86°Cm)=(1)(1.86°Cm)(m)(1)(1.86°Cm)m=25°C(1)(1.86°Cm)

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Problem Details

What volume of ethylene glycol (C2H6O2), 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/cm3, and the density of water is 1.00 g/cm3.)

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

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.

What professor is this problem relevant for?

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

What textbook is this problem found in?

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