V Data Analysis a The actual mass of the precipitates were far less than the

V data analysis a the actual mass of the precipitates

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and exhibited the same characteristics as the mixture created in part IA. V. Data Analysis a. The actual mass of the precipitates were far less than the predicted. This may have been because: i. Some amount of precipitate was not filtered and captured ii. Improper measuring of reactants iii. Loss of precipitate in transfer between locations iv. Unreacted ions in supernatant b. By calculation, all KIO 3 (aq) should have been consumed in the making of Ca(IO 3 ) 2 (s). However, the test for Ca 2+ showed positive. This may be because there were unreacted calcium ions in the mixture, which also explains why there was a discrepancy between the expected mass of precipitate and the actual mass. c. The observations seen in part IV were expected. In part IA, both solutions containing varying amounts of Ca(NO 3 ) 2 (aq) and KIO 3 (aq) turned a milky white/ cloudy color. The products of the reaction in part IV did the same. Part IV took longer because there was a greater amount of KIO 3 (aq) which required a greater amount of Ca(NO 3 ) 2 (aq). IV. Interpretation a. In this experiment the explanation to best fit the data is this: Ca(NO 3 ) 2 (aq) and KIO 3 (aq) combine to produce a solid and a liquid. Although KIO 3 (aq) is the limiting reactant, it was not completely consumed in this experiment. This left Ca 2+ (aq) and IO 3 - (aq) in the supernatant and caused a lower precipitate yield than expected.
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Conclusion This experiment showed that the solubility for Ca(NO 3 ) 2 (aq) is conditional; further inquiry is required to discern what these conditions are. Some ions were left undissolved in the supernatant which caused a low precipitate yield that differed from the expectation. Even with KIO 3 (aq) limiting the expected precipitate yield to .0487 grams, the actual yield was nearly 50 times smaller than expected yield.
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