Problem: A solution containing equal masses of glycerol (C3H8O3) and water has a density of 1.10 g/mL. Calculate the molarity of glycerol in the solution.

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FREE Expert Solution

We’re being asked to calculate the molarity (M) of glycerol (C3H8O3) in a solution. Recall that molarity is the ratio of the moles of solute and the volume of solution (in liters). In other words: We first need to determine the number of moles of C3H8O3. Assuming that we have 100 g of solution, this means we have 50 g of C3H8O3 and 50 g H2O.

To find the moles of C3H8O3, we’ll need its molar mass. The molar mass of C3H8O3 is:

C3H8O3     3 C × 12 g/mol C = 36 g/mol

8 H × 1 g/mol H = 8 g/mol

3 O × 61 g/mol O = 48 g/mol

Sum = 92 g/mol

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Problem Details

A solution containing equal masses of glycerol (C3H8O3) and water has a density of 1.10 g/mL. Calculate the molarity of glycerol in the solution.

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

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Based on our data, we think this problem is relevant for Professor Davis' class at UCF.