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HYDRATES OF COPPER SULFATE AND THE UNKNOWN LIQUID
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Introduction
This experiment was done to learn about true hydrates and the reactions that take place under different circumstances. It was hypothesized that the heating of copper sulfate would create an unknown liquid in a test tube and that unknown liquid would be sufficient to test for its identity. The hydrate that was used in this experiment was copper sulfate.
Methods
At the beginning of this experiment,.77grams of copper sulfate was heated and the liquid that developed due to the heating was allowed to evaporate. After the copper sulfate was heated and dried it was allowed to cool. At that time, it was measured again. Those results were used to design the second part of the experiment so that the appropriate amount of copper sulfate would be used. After the dry copper sulfate was cooled and measured, deionized water was added to the substance and the reaction was observed.
During the second part of this experiment, a piece of tubing was heated and bent into an "L" shape. This tube was placed in a rubber stopper. The rubber stopper with the tube was placed in a test tube that contained 18.06 grams of copper sulfate. The other end of the stopper was placed in a small test tube in order to collect the liquid that was generated by the experiment. The test tube and its contents were held above a lit Bunsen burner in order to heat the copper sulfate. While the copper sulfate's temperature rose, an unknown liquid began to evaporate from the substance. This liquid was condensed and collected in the test tube that the opposite end of the "L" shaped tube was placed in. When there was no longer any moisture present in the copper sulfate test tube, it was allowed to cool. The test tube with the copper sulfate was weighed again. The liquid that was collected was allowed to cool. The liquid was weighed and measured. The liquid was then heated to check its boiling point in order to detect its identity.
The third step of this experiment was done in order to check the results of the boiling point of the unknown liquid. Deionized water was heated and its temperature was measured using the same thermometer that was used to read the temperature of the unknown liquid.
Results
Amount of copper sulfate at beginning, grams Amount of copper sulfate recovered, grams Loss, grams Percent loss Liquid collected g and mL Density of the unknown liquid Boiling point of unknown liquid
Test #1 .77 .55 . % X X X
Test # 18.06 1.6 5.7 % 5.06g/ 5.0mL .7 g/mL 4 C
During the first test .77 grams of copper sulfate was used and .55 grams of copper sulfate was recovered after the experiment. There was a loss of . grams. It was found to be a % loss (Example ./.77 ᠐ 100 = %). In the second part of the experiment 18.06 grams of copper sulfate was heated and 1.6 grams was recovered. There was 5.7 grams lost. That was calculated to be a % loss. There was 5.0mL of liquid recovered in this process. It was found to weigh 5.06 grams. The density was calculated to be .7 g/mL (example 5.06g/5.0mL=density). The unknown liquids boiling point was found to be 4 degrees Celsius. The liquid was light blue and a pungent smell was noticed.
The same thermometer that was used to measure the temperature of the unknown liquid water was also used to measure the deionized water. The deionized water had a boiling point of 7 degrees Celsius.
Discussion
The chemical formula for this reactant is CuSO•5H0 so the liquid that condenses in the upper part of the test tube due to the heating of the reactant should be H0; however, the liquid that was recovered had a light blue tint and a pungent odor was noticed. The boiling point for the unknown liquid was three degrees Celsius less than the boiling point of H0, also H0does not have a pungent smell nor does it have a light blue tint; in fact, it is a substance that appears to be clear. It is apparent that some of the copper sulfate got into the liquid that was being recovered. This more than likely happened during the heating process, and it was because the tube was pointed downward instead of pointing it slightly up so that the copper sulfate would not run down into the liquid. The liquid came from the copper sulfate while it was being heated. While the copper sulfate was being heated it changed color. It went from a rich dark blue to a light blue color. This color change was due to the evaporation of the H0 from the copper sulfate. When all the liquid had been recovered and the copper sulfate was cool, a drop of deionized water was added to the copper sulfate. When this was done the copper sulfate immediately turned back into the rich dark blue color it was when the experiment began. The material appeared dry even though the deionized water was added to it. This shows that copper sulfate is a true hydrate.
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