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31 de ene. de 2021 · Students measure the mass of copper sulfate before and after dehydration and then figure out what happened to the mass to cause the change. By collecting multiple measurements as a clas...
10 de oct. de 2014 · No, it is not a chemical change! Copper sulfate ($\ce{CuSO4.5H2O}$) is a hygroscopic material. That means it readily co-ordinates with water. Hydrous $\ce{CuSO4}$ is not a bond. Therefore, when you heat copper sulfate crystals, the water evaporates leaving behind anhydrous copper sulfate which is white in colour.
Students remove the water of crystallisation from hydrated copper (II) sulfate by heating. Condensing the vapour produced in a second test tube collects the water. The white anhydrous copper (II) sulfate is then rehydrated and the blue colour returns.
Heat the crucible on the bunsen burner while stirring the copper sulfate with the scoopula. It will take about 5 minutes to drive off the water. The dried Copper sulfate has a tendancy to stick to the sides of the crucible and needs to be moved around to dry effectively.
Copper (II) sulfate is an inorganic compound with the chemical formula Cu SO 4. It forms hydrates CuSO4·nH2O, where n can range from 1 to 7. The pentahydrate ( n = 5), a bright blue crystal, is the most commonly encountered hydrate of copper (II) sulfate, [10] while its anhydrous form is white. [11]
17 de jul. de 2012 · A demonstration of dehydrating a sample of Copper Sulfate, as per the example from calculating percent compositions from the text - also mentioned in the previous video.
COPPER SULFATE PENTAHYDRATE can be dehydrated by heating. Serves as a weak oxidizing agent. Causes hydroxylamine to ignite. Gains water readily. The hydrated salt is vigorously reduced by hydroxylamine [Mellor 8:292(1946-1947)]. Both forms are incompatible with finely powdered metals.
