# Problem: An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d = 1.114 g/mL; ℳ = 62.07 g/mol) and water (d = 1.00 g/mL) at 20°C. The density of the mixture is 1.070 g/mL. Express the concentration of ethylene glycol as:(c) Molarity

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###### FREE Expert Solution

We're being asked to calculate the molarity of the ethylene glycol solution.

Recall molarity:

The mixture is made by mixing equal volumes of ethylene glycol and water → we can assume any volume:

Assuming: volume solution = 100 L

volume ethylene glycol = 50 L
volume water = 50 L

We're going to calculate the molarity of the solution using the following steps:

Step 1: Calculate moles of ethylene glycol (e.g.)
Step 2: Calculate the molarity of the solution

90% (10 ratings)
###### Problem Details

An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d = 1.114 g/mL; ℳ = 62.07 g/mol) and water (d = 1.00 g/mL) at 20°C. The density of the mixture is 1.070 g/mL. Express the concentration of ethylene glycol as:

(c) Molarity

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 Calculate Molarity concept. You can view video lessons to learn Calculate Molarity Or if you need more Calculate Molarity practice, you can also practice Calculate Molarity practice problems .

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Based on our data, we think this problem is relevant for Professor Scerri's class at UCLA.

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