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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]
It is easily recognisable, due to its distinct red-orange color. Copper also has a range of different organic and inorganic salts , having varying oxidation states ranging from (0,I) to (III). These salts (mostly the (II) salts) are often blue to green in color, rather than the orange color copper is known for.
Copper(II) sulfate, CuSO 4, a common, greenish blue compound used as a fungicide and herbicide; Copper(I) sulfate, Cu 2 SO 4, an unstable white solid which is ...
Chalcanthite can also dye materials blue when dissolved in water, and has a peculiarly sweet and metallic taste, although consuming it can induce dangerous copper poisoning. Crystal structure of chalcanthite Color code::Copper, Cu: brown :Sulfur, S: olive :Oxygen, O: red :Cell: cyan
why does this substance change color from blue to green when water is added? It shouldn't. Copper (II) Sulfate forms a light blue solution. If the water has a lot of chloride ions in it, a complex ion may be formed that would make the solution green. --24.16.154.50 00:05, 12 January 2007 (UTC)
Specifically, using Benedict's reagent and Fehling's solution the presence of the sugar is signaled by a color change from blue Cu(II) to reddish copper(I) oxide. [4] Schweizer's reagent and related complexes with ethylenediamine and other amines dissolve cellulose. [5] Amino acids such as cystine form very stable chelate complexes with copper(II).
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Predicting the color of a compound can be extremely complicated. Some examples include: Cobalt chloride is pink or blue depending on the state of hydration (blue dry, pink with water) so it is used as a moisture indicator in silica gel. Zinc oxide is white, but at higher temperatures becomes yellow, returning to white as it cools.