Project 11 Identification Properties And Synthesis Of An Unknown Compound

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Discussion There were four goals for Project 11: Identification, Properties, and Synthesis of an Unknown Ionic Compound. The first goal was to identify the unknown compound, the second goal was to determine the reactivity of the compound, the third goal was to determine the quantitative solubility of the compound in water, and the fourth goal was to find the percent yield of a product from a reaction involving the unknown compound.
Determining the identity of the unknown compound was achieved by performing a variety of tests for the physical properties of the substance. Some of these properties, such as melting point and chemical structure, could be discovered by making a few immediate observations of the substance. The unknown compound
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Also, the particles of the substance looked like crystals, so it could be inferred that the compound had a lattice structure. Lastly, the unknown compound looked very similar to salt, which has a formula of NaCl, because it was a white, shiny solid. It was very likely then that our unknown compound would have properties similar to salt.
On the first day of lab, tests for qualitative solubility, conductivity, pH, cations, and anions were performed. After performing the qualitative solubility test, it was apparent that the unknown compound dissolved in water, but not toluene or acetone. Since the unknown compound dissolved in water, it was most likely ionic or polar. However, it did not dissolve in acetone, a polar solvent, so the compound had to be ionic.1 The conductivity test revealed that a solution of the compound can conduct electricity. Since all soluble ionic compounds are strong electrolytes, which conduct electricity in solution, this test confirmed that the unknown compound was ionic.2 The pH test revealed that the unknown compound was slightly acidic because the pH strip had a slightly red
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A quantitative analysis determines the amounts or concentrations of the substances in a sample using chemical reactions and stoichiometric calculations.5 The unknown compound (KCl) and the “known” KCl were reacted with silver nitrate (Ag(NO3)2) to produce a precipitate (AgCl2) that could be measured after performing vacuum filtration. The actual yields of the “unknown” KCl reactions and “known” KCl reactions should be very similar because based on our identification, they are the same compound. The grams of precipitate recovered for both the “unknown” KCl and “known” KCl reactions ranged from 0.694 grams to 1.054 grams. However, the theoretical yield of AgCl2 in this reaction was only supposed to be 0.600 grams, so all of the percent yields calculated in the experiment are above 100%. This indicates that a lot of error occurred during the quantitative

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