Three different versions! Placed crucible on mesh pad using tongs (from this point, the crucible was handled solely with tongs until the experiment concluded), and allowed to cool to room temperature. Copper/Iron Stoichiometry Grace Timler AB1 October 3, 2017 Abstract The techniques used in this lab are quantitative transfer and vacuum filtration with the reaction of 8.001 grams of copper (II) sulfate, CuSO4, and 2.0153 grams of iron powder, Fe. Through the use of a vacuum filtration system the mass of Cu was, Flame Test Lab Report cup' method. Hydrate: A compound that contains the water molecule. This is a student-centered, active learning lesson without lecture or notetaking! Use the information collected in lab found below to fill in the blanks for the gram amounts above: Use this picture to get the mass of the empty crucible and fill it in above. Rounded to the nearest integer, the ratio is 1:5. Distilled, Precipitation Reactions This was the same for all five trials. Materials: Tests tubes (small or medium size), watch glasses, crucible* and cover*, crucible tongs, clay triangle. Natural Gas Hydrates, Fourth Edition, provides a critical reference for engineers who are new to the field. Weigh and record the mass of the cooled crucible with its cover and content (anhydrous residue). The weight after cooling of the evap dish is constant. (8 points) 7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. On an analytical balance, weigh a pea-sized sample of each of the compounds below on separate clean and dry watch glasses. Set up the apparatus as shown (but without water in the receiving tube - this is to be collected during the experiment), placing about 5 g of powdered hydrated copper(II) sulfate in the test tube. The results for the heating, Title: Title of lab/experiment. Return the evaporating dish with the hydrate to the wire gauze. Answer: Compounds to be tested: \(\ce{Na2SO4*10H2O}\), \(\ce{FeCl3}\), \(\ce{KAl(SO4)2}\), \(\ce{CaCl2}\), \(\ce{CuSO4}\). 1.7: Experiment 6 - Hydration of Salt - Chemistry LibreTexts Send me a message, I'd love to hear from you! However, immediately after the first heating, It can be clearly seen that the heated copper sulfate has now transformed into a grainy and whitish-gray form. For each of the chemical compounds below, place a. dissolved is another. When dissolved in water, the anhydrous compound will have a color similar to that of the original hydrate even if it had changed color going from the hydrate to the anhydrous compound. The lab has an introduction to help students understand why they are doing the lab. They are very math intensive, and very conceptual in nature. Fill half of the flask with distilled water, add the stopper for the flask, and lightly shake the flask, until the copper sulfate pentahydrate fully dissolved. Compounds to be tested: Nickel (II) chloride, Cobalt (II) chloride, Sucrose, Calcium Carbonate, Barium chloride, Sodium tetraborate, Potassium chloride. Kieran Sidebotham Any time she touches the apparatus its under close supervision by myself. FEATURESGuided notes that have students listening to you instead of writing notes.Opt to use slides for all students and guid, This is the perfect companion to the popular chemistry lab: Determining the Formula of an Unknown Hydrate.
Murray's Bagels Nutrition Info,
Macnaughton Family Hawaii,
Proximal Tibiofibular Joint Instability,
Articles C
