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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]
Although magnesium bromide generated in situ from the reaction of Grignard reagents and copper(I) halides can serve this role (see above), external Lewis acids are also useful. In the presence of boron trifluoride etherate, organocopper complexes are able to add to sterically congested enones in moderate yield (effecting the same transformation ...
"It can also be prepared by electrolysis of magnesium sulfate [Epsom salts] solution at moderate voltage with a copper anode: this reaction produces hydrogen, copper sulfate solution, and copper hydroxide precipitate." what happens to the magnesium? MgSO4(aq) + Cu(S) --dc--> h2(g) + Mg(OH)2(s) + CuSO4(aq) would make more sense.
pyrometallurgical extraction using magnesium, or less commonly other alkali metals, hydrogen or calcium in the Kroll process: Manganese Mn Mn 2+ reacts with acids; very poor reaction with steam smelting with coke: Zinc Zn Zn 2+ Chromium Cr Cr 3+ aluminothermic reaction: Iron Fe Fe 2+ smelting with coke: Cadmium Cd Cd 2+ Cobalt Co Co 2+ Nickel ...
Magnesium sulfate or magnesium sulphate is a chemical compound, a salt with the formula MgSO 4, consisting of magnesium cations Mg 2+ (20.19% by mass) and sulfate anions SO 2− 4. It is a white crystalline solid , soluble in water but not in ethanol .
Like magnesium oxide, it will generate a basic carbonate when placed in the air. [3] Magnesium sulfide can be produced by the reaction of magnesium and hydrogen sulfide, or by the reaction of magnesium sulfate and carbon disulfide at high temperature: [6] Mg + H 2 S → MgS + H 2 3 MgSO 4 + 4 CS 2 → 3 MgS + 4 COS + 4 SO 2
Consider the Galvanic cell shown in the adjacent image: it is constructed with a piece of zinc (Zn) submerged in a solution of zinc sulfate (ZnSO 4) and a piece of copper (Cu) submerged in a solution of copper(II) sulfate (CuSO 4). The overall reaction is:
The flame test carried out on a copper halide. The characteristic bluish-green color of the flame is due to the copper. A flame test is relatively quick test for the presence of some elements in a sample. The technique is archaic and of questionable reliability, but once was a component of qualitative inorganic analysis.