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Copper(II) nitrate describes any member of the family of inorganic compounds with the formula Cu(NO 3) 2 (H 2 O) x.The hydrates are hygroscopic blue solids. Anhydrous copper nitrate forms blue-green crystals and sublimes in a vacuum at 150-200 °C.
2 NaOH + CuO + H 2 O → Na 2 [Cu(OH) 4] It can also be reduced to copper metal using hydrogen, carbon monoxide, and carbon: CuO + H 2 → Cu + H 2 O CuO + CO → Cu + CO 2 2 CuO + C → 2Cu + CO 2. When cupric oxide is substituted for iron oxide in thermite the resulting mixture is a low explosive, not an incendiary.
Copper azide can be prepared by a metathesis reaction between water-soluble sources of Cu 2+ and azide ions. (Spectator ions omitted in reaction below). Cu 2+ + 2 N − 3 → Cu(N 3) 2. It can be destroyed by concentrated nitric acid to form non-explosive products, these being nitrogen, nitrogen oxides and copper(II) nitrate.
Print/export Download as PDF; Printable version; In other projects Wikidata item; Appearance. move to sidebar hide ... Ag 5 Cu 2 (NO 3)(SeO 3) 4: 1326.26 triclinic P 1:
Copper(II) hydroxide is the hydroxide of copper with the chemical formula of Cu(OH) 2.It is a pale greenish blue or bluish green solid. Some forms of copper(II) hydroxide are sold as "stabilized" copper(II) hydroxide, although they likely consist of a mixture of copper(II) carbonate and hydroxide.
The tetrahydrate consists of discrete, octahedral [(H 2 O) 4 Co(NO 3) 2] molecules. The hexahydrate is better described as hexaaquacobalt(II) nitrate, [Co(OH 2) 6][NO 3] 2, as it consists of discrete [Co(OH 2) 6] 2+ and [NO 3] − ions. [5] Above 55 °C, the hexahydrate converts to the trihydrate and at higher temperatures to the monohydrate. [2]