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 = 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.
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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