The Depression of Frozen Point

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The Depression of Frozen Point The boiling point and the freezing point both refer to colligative properties; in other words, the individuality of each particle is not as significant as the number of dissolved particles in a solution. In a solution, the boiling point increases and the freezing point decreases when the concentration of particles increases; this means that the change in normal boiling point as well as freezing point of water is connected to the increase of particles. Throughout the experiment, calculating the freezing point depression constant of solvent was a significant process. Observing the co-relation between the sugar concentration and freezing point was important too. In addition, the freezing point of the same solution for sugar and salt was compared. The equation: ΔT= iKfm shows the relationship for the freezing point; which ΔT is the change of temperature from the original freezing point, i is the number(s) of particle(s) (van’t Hoff factor), Kf is the freezing point depression constant for the solvent, and m is the molality of solution. The experiment should be able to prove that one of the molalities of sugar solution will equal to the molality of salt. Procedures The experimenters began by calculating the concentrations of each sugar solution (g/mL). Results Information such as data, graphs, calculations, etc. are recorded in Discussion The sugar concentration should change with the higher depression. One of the sugar concentration solutions should have an equal molality to salt solution. The biggest flaw of the experiment was that the experimenters did not match any masses of sugar with the mass of salt. The mass of salt was 0.3197g with the molality of 1.092. However, all sugar concentration solutions weighed 0.985g with

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