Cation Flame Test Lab Report

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In Part A of the experiment, the Unknown Substance #4 was found to contain Silver. Since no precipitate was formed in Step 6 of the experiment, it was confirmed that there was no presence of lead. Step 8 verified that the unknown solution contained Silver, with the formation of the white AgCl precipitate. Silver was reasonable since it was confirmed that it was not Lead. Part B of the experiment resulted in the identification of Barium. The presence of Barium was confirmed in Step 13, with the formation of the white BaSO4 precipitates in the orange solution. The unknown solution was further tested to avoid a false positive confirmation of Calcium in Step 14. No precipitate was formed so the solution in the 1M K2C2O4 so the Barium was once again verified. Barium was reasonable since it had been…show more content…
After a metal salt is added to a hot flame, it shifts from the excited state to its ground state, displaying a discrete spectrum of light. For example, Barium Chloride will emit a yellow color, whereas Lithium Chloride emits a dark red color. However, the cation flame test is limited in that if multiple cations are present, the results can be altered. The result of an impure solution can cause the mixing of emitted wavelengths and colors. Alternatively, one cation can potentially conceal the identity of the others.3 If this experiment were to have been repeated, micropipettes would be used instead of the standard pipettes to increase the accuracy when withdrawing fluids. This would substantially decrease the degree of errors due to incorrect measurements. Additionally, the centrifuges would be replaced with new machines since the previous centrifuges caused a few test tubes to break, even though the solutions had been evenly balanced by weight. More caution may also be needed when balancing the centrifuges to prevent future
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