Why Does The Ammonium Chloride Increase The Amount Of Solute?
The mass of urea was normalized so that it could become the equivalent of what it would’ve been in the larger solvent as numbered in Data Table 4. There wasn’t much difference between the corrected number of moles and grams of urea and the amount of urea used originally used in the experiment, so the ammonium chloride will be primarily compared to the corrected amount of urea to make sure that the amount of solvent is equal. Graph 1 and 5 and Data Table 2 show that the mass of solutes were overall very similar: 8.735 grams of ammonium chloride and 8.99 grams of urea. Overall, this experiment proved that the freezing point depression is a colligative property that depends on the number of moles of solute but not on the identity of the solute.
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As displayed on Graph 2 and Graph 6 and typed in Data Table 3 and 4, the moles of solute for ammonium chloride and the corrected moles of solute for urea were very close: .1627 moles of ammonium chloride and .1492 moles of urea. Even though the amount of moles was very similar, there is clearly a stark difference in the change in temperature when comparing Graph 2 and 6: When all of the moles of each solute were added to each beaker, the final change in temperature for ammonium chloride was nearly double that of the final change in temperature for urea. As shown in Data Table 3 and 4, the final change in temperature for ammonium chloride was 4.74 °C, and the final change in temperature for urea was 2.09 °C. To cause these results, ammonium chloride, which is a salt of a weak base, more than likely dissociated into ammonium ions and chlorine ions, resulting in twice as many more particles in solution than urea, which probably doesn’t dissociate much or at all, in the water/ice
As displayed on Graph 2 and Graph 6 and typed in Data Table 3 and 4, the moles of solute for ammonium chloride and the corrected moles of solute for urea were very close: .1627 moles of ammonium chloride and .1492 moles of urea. Even though the amount of moles was very similar, there is clearly a stark difference in the change in temperature when comparing Graph 2 and 6: When all of the moles of each solute were added to each beaker, the final change in temperature for ammonium chloride was nearly double that of the final change in temperature for urea. As shown in Data Table 3 and 4, the final change in temperature for ammonium chloride was 4.74 °C, and the final change in temperature for urea was 2.09 °C. To cause these results, ammonium chloride, which is a salt of a weak base, more than likely dissociated into ammonium ions and chlorine ions, resulting in twice as many more particles in solution than urea, which probably doesn’t dissociate much or at all, in the water/ice