Hydrates Formal Lab Report.docx

Nickel sulfate before heating the nickel sulfate

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Nickel Sulfate: Before heating, the nickel sulfate appeared as turquoise crystals. After the first heating, the crystals fused together. This compound tested as nonacidic. After the second heating, the nickel sulfate became yellow and bubble on the outside, and on the inside, there was green crystal fused together. After cooling, the appearance did not change. Copper Sulfate: Before heating, the copper sulfate consisted of blue and white crystals. After the first heating, some of the crystals changed colors to yellow and green. This compound is nonacidic. After the second heating, the crystals turned brown and white, with the blue almost completely going away. The same remained after the compound cooled. Data: Part 1: Mass of crucible and lid 31.167 g Mass of crucible, lid, and barium chloride dihydrate 32.828 g Mass of barium chloride dihydrate 1.661 g Mass of crucible, lid, and contents after initial heating 32.579 g Mass of crucible, lid, and contents after second heating 32.579 g Mass of water lost 0.249 g (32.828-32.579) Mass of anhydrous barium chloride 1.416 g Equation used to determine the mass of anhydrous barium chloride: 1.661 g BaCl 2 2 H 2 O × 1 mole BaCl 2 2 H 2 O 244.3 gBaC l 2 2 H 2 O × 1 moleBaCl 2 1 mole BaCl 2 2 H 2 O × 208.3 gBaCl 2 1 mole BaCl 2 = 1.416 gBaC l 2 Chemical equations for hydrates tested in Part 2: 2(CrCl 3 · 6H 2 O) Cr 2 O 3 + 6HCl + 9H 2 O CoCl 2 · 6H 2 O CoCl 2 + 6H 2 O NiSO 4 · 7H 2 O NiSO 4 + 7H 2 O CuSO 4 · 5H 2 O CuSO 4 + 5H 2 O
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Discussion: For part 1 of this experiment, it could be predicted that the mass of the barium chloride dihydrate would be reduced after going through the thermal decomposition reaction. This prediction can be made because the water in the dihydrate leaves the compound when it is heated and turns from liquid to gas. The mass of the water leaves the compound, and thus, the anhydrous barium chloride has a lesser mass. As far as determining the correct theoretical reaction equation, it could be assumed that the mass of either barium chloride or barium oxide would be very close to the mass found through weighing the anhydrous barium chloride. Thus, after finding which theoretical mass is closest, it can be deduced that the equation with the closest mass is the correct equation to represent the thermal decomposition reaction that occurred in the experiment. Generally, there is a percent error in place for the theoretical mass
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  • Spring '13
  • ABC
  • Barium, Copper(II) sulfate, barium chloride

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