Properties of Hydrates Essay

PurposeThe purpose of the Properties of Hydrates laboratory is to study provides, and be subject to identify them. This lab standardizedly focuses on observing the reversibility of hydration reactions by hydrolysis, and also testing substances for efflorescence of deliquescence.ProcedureA.Identification1. Place 0.5 gees of each colonial (Nickel Chloride, green Chloride, atomic number 11 Tetraborate, Sucrose, calcium Carbonate, and Barium Chloride) in a sm all in all juiceless test tube. 2. Heat gently with a burner flame and observe conservatively. If droplets of piss appear on the test tube it may be a furnish. Note the nature and subterfuge of the residue. 3. Let the tube cool, and try to disperse the residue in a some cm3 of pissing, warming if necessary. A straight hydrate will dissolve in urine supply supply, producing a color similar to that of the original hydrate. A carbohydrate will give off water, plainly tends to char. The residue will also often be a caramel color.B.Reversibility1. Gently heat a few crystals of about 0.3 grams of hydrated Cobalt(II) Chloride, CoCl2 x 6H2O in an evaporating bang until the color change appears to be complete 2. free the residue in the evaporating dish in a few cm3 of water from the wash bottle 3. Heat the residue to a boiling and carefully boil it to dryness. Note any color changes. 4. put up the evaporating dish on the lab bench and let it cool.C.Deliquescence and Efflorescence1. Place a few crystals of Na2CO3 x 10H2O, CaCl2, KAl(SO4)2 x 12 H20, and CuSO4 in an a separate evaporating dish next to the CoCl2 prepa going in office B. 2. To see weather the samples gained or lost clutch, weigh each of them on a top-loading balance and genius to the nearest hundredth. 3. Weight them again later on an hour to detect either changes in mass. 4. Observe the samples occasionally. Note any buildings in color and structure and degree of wetness.D. Percent of Water in Hydrate1. Clean crucible and its cover, and also make sure that crucible tongs are clean. Put over fire, and let cool. 2. Weight the crucible to the nearest thousandth. Handel with tongs 3. master a sample of an dark hydrate, and place about 1 gram in the crucible. 4. Weight the crucible, cover and sample on the balance. 5. Put the crucible on the clay triangle, with the cover off center to allow water vapor to escape. 6. Heat again, gently at first, and then with the bottom red for about 10 minutes. 7. Center the crucible cover, and let it cool to room temperature. 8. Weight the cooled crucible and with its cover and contents. 9. Examine the solid residue.10. Add water until the crucible it two thirds full. Warm gently if the residue doesnt right away dissolve. 11. Does the residue appear to be dissoluble?Waste Disposal advance of the Copper mixture, and the Aluminum mixture in the correct bowl to a lower place the waste hood. All of the acids and bases can be disposed of down the sink. If the compou nd isnt water soluble put in the organic container. chemic Principles in the Laboratory Experiment 6ConclusionThe purpose of the Properties of Hydrates lab was to be able to identify if a substance was a hydrate or not. In lab, experiments where conducted to see if a compound was a hydrate or not. In order for the compound to be deemed as a hydrate it had to1. Release water upon heating2. The anhydrous residue had to be water soluble3. Exhibit reversibilityIf, and only if the compound showed that it could exhibit all three of these properties, could it be distinguished a hydrate. In part A of the experiment, Nickel Chloride and Sodium Tetraborate were the only two compounds that were reliable hydrates. Both of these showed water residue when heating, where soluble in water after heating, and converted subscribe to it original color after performing the first two experiments. some of the other compounds had positive results for integrity or two test moreover not all three. F or example, Sucrose, when heated, water residue appeared on the test tube, and was soluble in water, but the compound didnt show reversibility.In part B of the experiment, CoCl2*6H2O was heated, dissolved, and then heated again to show that it was a true hydrate. When the Cobalt Chloride was heated, it turned from the color of fuchsia pink, to a light blue. And then after being dissolved into water, the compound turned back to its original color of fuchsia pink, demonstrating reversibility. The color change in this compound shows that by adding water to the anhydrous residue, that the same bonds that were broken my dehydrating the compound where reformed when adding water.In part C, four compound, plus the Cobalt Chloride mentioned above were tested for deliquescence, and efflorescence. Only one compound turned about to be efflorescent, which means that it lost water, which was Sodium Carbonate. The compounds mass before sitting out was 50.645g, after being unresolved to the condit ions of the laboratory for an hour, the sample weight 50.603g losing approximately 0.042g over the period of an hour. The Calcium Chloride (gained 0.258g), Copper Sulfate (gained 0.007g) and Cobalt Chloride (gained 0.068g) where all deliquescent, meaning that again mass enchantment sitting in the laboratory. The Potassium Aluminum sulfate, exhibited stability while sitting out for an hour, neither gaining nor losing mass.For part D of the experiment, the percent of water in the unknown hydrate was %12.290. The closet percent of the given facts of the unknown was Barium chloride (BaCl2*2H2O), which has %14.8 water in it. This percent was found by apply the formula below % water in hydrate=(mass of water in hydrate/mass of the entire hydrate)The wide range of difference surrounded by the percent of the given and the unknown could have been due to the fact that at that place was wood debris in the unknown sample . This could have throw off the essence of water present in the samp le, and messed up the amount of water able to evaporate.