Lab Report- Freezing Point Depression.docx - FREEZING POINT DEPRESSION LAURIC ACID SOPHIA TORRES CHM 113 R2 Abstract The Kf values of Lauric Acid

Lab Report- Freezing Point Depression.docx - FREEZING POINT...

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FREEZING POINT DEPRESSION: LAURIC ACID S OPHIA T ORRES CHM 113 R2 Abstract The Kf values of Lauric Acid solutions with different amounts of Benzoic acid (solute) were found. The solution containing 0.750 g Benzoic acid and 8.00 g Lauric acid was found to have a Kf value of 52.1. The solution containing 1.50 g Benzoic acid and 8.00 g Lauric acid was found to have a Kf value of 26.1. The average Kf value between the two solutions was 39.1. Introduction The molecules of a substance become very closely packed and form a certain arrangement when the substance freezes. Impurities can sometimes interfere with the molecular interactions; as a result, the temperature must be lower in order for the system to solidify. The amount the freezing point must be lowered is given by the equation T = K f m . T is the amount the freezing point has been lowered in C , m is the molality of the solution, K f is the freezing point depression constant for the solvent. Molality is the number of moles divided by the mass of the solvent, in contrast to molarity which is the number of moles divided by the volume of the solution. Molality is used in this equation because the value remains the same regardless of temperature, whereas volume, which affects molarity, is affected by temperature changes. The solution in this experiment is a solute (benzoic acid) in the solvent lauric acid.
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