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Copper(II) sulfate is an inorganic compound with the chemical formula Cu SO 4.It forms hydrates CuSO 4 ·nH 2 O, 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]
Molecular weight (M.W.) (for molecular compounds) and formula weight (F.W.) (for non-molecular compounds), are older terms for what is now more correctly called the relative molar mass (M r). [8] This is a dimensionless quantity (i.e., a pure number, without units) equal to the molar mass divided by the molar mass constant .
CuSO 4 · 5 H 2 O loses 4 H 2 O at 110 C, loses 5 H 2 O at 150 C; CuSO 4 decomposes to CuO at 650 C; CuO decomposes at 1026 C; The above description is right. You get CuSO4 -> CuO + SO3 as it decomposes. First of all, I've done this one before and can attest that you can't get copper. Second, the current equation has O2 and Cu metal as products.
The percentage of the weight of CuSO 4 to the weight of water employed determines the concentration of the mixture. Thus a 1% Bordeaux mixture, which is typical, would have the formula 1:1:100, with the first "1" representing 1 kg CuSO 4 (pentahydrated), the second representing 1 kg hydrated lime, and the 100 representing 100 litres (100 kg) water.
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