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29 Σεπ 2024 · The anhydrous salt is copper (II) sulfate. This is usually seen as white crystals / powder. Adding water to the anhydrous salt forms the hydrated copper (II) sulfate pentahydrate, CuSO 4 •5H 2 O. This reaction is highly exothermic. The forward reaction is exothermic and the reverse reaction is endothermic. Another example is cobalt (II) chloride:
Formula of a Hydrate (\(\text{Anhydrous Solid}\ce{*}x\ce{H2O}\)) The formula of a hydrate can be determined by dehydrating a known mass of the hydrate, then comparing the masses of the original hydrate and the resulting anhydrous solid.
7 Ιουν 2024 · A compound which doesn’t contain water of crystallisation is called an anhydrous compound. E.g. anhydrous copper (II) sulfate is CuSO 4. A compound can be hydrated to different degrees. E.g. cobalt (II) chloride can be hydrated by six or two water molecules. CoCl 2 ∙ 6H 2 O or CoCl 2 ∙ 2H 2 O.
After heating, the mass of the anhydrous compound is found to be 3.22 g. Determine the formula of the hydrate and then write out the name of the hydrate. Solution: 1) Determine mass of water driven off: 4.31 − 3.22 = 1.09 g of water. 2) Determine moles of Na 2 CO 3 and water: Na 2 CO 3---> 3.22 g / 105.988 g/mol = 0.0304 mol
22 Σεπ 2021 · The formula of a hydrate can be determined by dehydrating a known mass of the hydrate, then comparing the masses of the original hydrate and the resulting anhydrous solid. The mass of water evaporated is obtained by subtracting the mass of the anhydrous solid from the mass of the original hydrate (\ref{3}):
We can find the percent of water in a hydrate experimentally by accurately determining the mass of the hydrate and the mass of the anhydrous salt. The difference in mass is due to the water lost by the hydrate.
We can use difference in the mass between the hydrated and anhydrous compound to calculate the mass of water of crystallisation removed by heating.
