Hydrate Laboratory

Hydrate Laboratory

A hydrate is an ionic compound with water molecules loosely bonded to its crystal structure. The water is in a specific ratio to each formula unit of the salt. An example wouldbe CuSO4 . 5H2O, this ionic compound called copper sulfate indicates that there are five water molecules for every formula unit of CuSO4. In this chemical formula, a dot is commonly used to separatethe formula of the anhydrous salt, (which represents the salt without water), from the number of water molecules. Hydrates can usually be converted to the anhydrous form by heating: Hydrated salt →anhydrous salt + water (CuSO4 • 5H20 → CuSO4 + 5H20). Hence it is possible to determine the percentage of water present in a hydrated salt by determining the amount of mass lost in heating.Additionally to be able of doing this experiment you will have to find the molar mass of the ionic compound, to do so you find the mass of the copper sulfate and then add 5 times the mass of water to it,(63.55+32.07+4(16.00)+5(18.02)= 249.72g/mol).In order to make this experiment you will need: 500 g of copper (II) Sulfate, a triple beam balance, an evaporating dish, tongs, a hot plate, and a Scoopula.The procedures need to be followed in the chronological order. For the first step, clean the evaporating dish, and find its mass using a triple beam balance. Then, take a scoop of the hydrate CuSO4 •5H2O, and put it into the evaporating dish and find its mass again. Now put the evaporating dish on a hot plate and heat it under moderate heat for 10 minutes, or until there is no more water left. Thenlet the evaporating dish cool down, and find its mass again. By heating the evaporating dish the water of the hydrate will evaporate and you will be left with the anhydrous, which is the copper (II)Sulfate. When finished, scrape your anhydrous salt into the disposal container and clean up your area. To conclude write your measurements on the table data. Remember to find the mass of the water...