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A 0.520 g sample of an unknown nonelectrolyte compound is dissolved in 4.12 g of lauric acid (Kf = 3.90 °C/m). The freezing point depression is determine to be 4.20 °C. What is the molar mass of the compound?

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Answer:

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Explanation:

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The molar mass of the unknown nonelectrolyte compound is

Using the formula;

∆T = K m i

Where;

K = freezing point depression constant

m = molality of the solution

i = Van't Hoft factor

Note that i = 1 since the compound is a nonelectrolyte.

To find molality;

Number of moles = 0.520 g/Molar mass

Let the molar mass of the unknown compound be MM

Number of moles = 0.520 g/MM

Number of kilograms of solvent = 4.12 g/1000 = 0.00412 Kg

Molality = 0.520 g/MM * 1/0.00412 Kg

Freezing point depression is 4.20 °C

To find the molar mass of the compound;

4.20 °C = 3.90 °C/m *  0.520 g/MM * 1/0.00412 Kg

4.20  = 492.23/MM

MM = 492.23/4.20

MM = 117.19 g/mol

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