When calculating the freezing point of a solution, we’re walking to use the equation for Freezing suggest Depression.

You are watching: Freezing point of lauric acid in celsius

∆Tf=i·Kf·m

∆Tf = change in freezing point = Tf pure solvent –Tf solutionKf = freezing point depression constanti = van\" t Hoff aspect of the solute = no. The ionsm = molality

Part a.)We\"re gift asked to calculate molality (m), in mol/kg. The Kf value for lauric mountain is 3.9°C•kg/mol.


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Using freezing point depression to find molecular weight

Mass that Lauric mountain (g) 8.003

Mass of benzoic mountain (g) 1.010

Freezing temperature the pure lauric acid (C°) 43.84

Freezing temperature that the benzoic acid-lauric acid mixture (C°) 39.05

a. Calculate molality (m), in mol/kg, making use of the formulaΔt = Kf *m. The Kf worth for lauric acid is 3.9°C•kg/mol.

b. Calculate moles of benzoic mountain solute, utilizing the molality and the mass (in kg) of lauric mountain solvent.

c. Calculation the speculative molecular weight of benzoic acid, in g/mol.

d. Recognize the welcomed molecular load of benzoic acid from that is formula, C6H5COOH.

e. Calculate the percent discrepancy between the experimental and accepted values.


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