Copper II sulfate

A characteristic property of an aldehyde function is its sensitivity to oxidation A solu tion of copper(II) sulfate as its citrate complex (Benedict s reagent) is capable of oxi dizing aliphatic aldehydes to the corresponding carboxylic acid... 

Fehlmgs solution a tartrate complex of copper(II) sulfate has also been used as a test for reducing sugars... 

Use of Centered Period. A centered period is used to denote water of hydration, other solvates, and addition compounds for example, CUSO4 SHjO, copper(II) sulfate 5-water (or pen-tahydrate). 

Hydroxylamine Barium oxide and peroxide, carbonyls, chlorine, copper(II) sulfate, dichromates, lead dioxide, phosphorus trichloride and pentachloride, permanganates, pyridine, sodium, zinc... 

Gopper(II) Sulfates. Copper(II) sulfate pentahydrate [7758-99-8] CuS04-5H20, occurs in nature as the blue triclinic crystalline mineral chalcanthite [13817-21 -5]. It is the most common commercial compound of copper. The pentahydrate slowly effloresces in low humidity or above 30.6°C. Above 88°C dehydration occurs rapidly. 

Copper(II) sulfate monohydrate [10257-54-2] CuS04-H2 0, which is almost white in color, is hygroscopic and packaging must contain moisture barriers. This product is produced by dehydration of the pentahydrate at 120—150°C. Trituration of stoichiometric quantities of copper(II) oxide and sulfuric acid can be used to prepare a material of limited purity. The advantages of the monohydrate as opposed to the pentahydrate are lowered freight cost and quickness of solubilization. However, these advantages are offset by the dustiness of the product and probably less than one percent of copper sulfate is used in the monohydrate form. 

Anhydrous copper(II) sulfate [7758-98-7] is a gray to white rhombic crystal and occurs in nature as the mineral hydrocyanite. CuSO is hygroscopic. It is produced by careful dehydration of the pentahydrate at 250°C. An impure product can also be produced from copper metal and hot sulfuric acid ... 

There are four basic sulfates that can be identified by potentiometric titration using sodium carbonate (39,40) langite [1318-78-17, CuSO -3Cu(OH)2 H2 i brochantite [12068-81 -4] CuSO -3Cu(OH)2 antedite [12019-54-4] CuSO -2Cu(OH)2 and CuS0 -Cu0-2Cu(0H)2-xH20. The basic copper(II) sulfate that is available commercially is known as the tribasic copper sulfate [12068-81 ] CuS04-3Cu(0H)2, which occurs as the green monoclinic mineral brochantite. This material is essentially insoluble in water, but dissolves readily in cold dilute mineral acids, warm acetic acid, and ammonia solutions. 

Tribasic coppersulfate is usually prepared by reaction of sodium carbonate and copper sulfate. As the temperature of the reaction contents increases so does the size of the resulting particle. For use as a crop fungicide, intermediate (40—60°C) temperatures are used to obtain a fine particle. When lower temperatures are used to precipitate basic copper(II) sulfate, products high in sulfate and water of hydration are obtained. 

Copper (II) sulfate (anhydrous). Suitable for esters and alcohols. Preferable to sodium sulfate in cases where solvents are sparingly soluble in water (for example, benzene or toluene). 

Dialing solution Dissolve 1.5 g copper(II) sulfate pentahydrate in a few milliliters of water and make up to 100 ml with methanol. 

For the determination of sterols and their esters the chromatogram is immersed in a 10% aqueous copper(II) sulfate solution and then heated to 105°C for 30 min. In this case green-yellow fluorescent chromatogram zones are visible in long-wavelength UV light (X = 365 nm) [6]. 

A mixture of 10% aqueous copper(II) sulfate solution and 25% ammonia solution (100 -I-15) is recommended as spray solution for the detection of diuretics. 

In alkaline solution biuret, HN(CONH2)2 reacts with copper(II) sulfate to give a characteristic violet colour due to the formation of the complexes [Cu2(/l-OH)2(NHCONHCONH)4] (Fig. 28.6a) and [Cu(NHCONHCONH)2] . This is the basis of the biuret test in which an excess of NaOH solution is added to the unknown material together with a little CUSO4 soln a violet colour indicates the presence of a protein or other compound containing a peptide linkage. 

Cupri-. cupric, copper(II). -azetst, n. cupric acetate, copper(II) acetate, -carbonat, n. cupric carbonate, copper(II) carbonate, -chlorid, n. cupric chloride, copper(II) chloride. -hydroxyd, n. cupric hydroxide, cop-per(II) hydroxide. -ion, n. cupric ion, copper(II) ion. -ozalat, n. cupric oxalate, copper(II) oxalate, -oxyd, n. cupric oxide, copper(II) oxide. -salz, n. cupric salt, copper(II) salt, -suifat, n. cupric sulfate. copper(II) sulfate, -sulfid, n. cupric sulfide, copper(II) sulfide, -verbihdung, /. cupric compound, copper(II) compound, -wein-saure, /. cupritartaric acid. 

Copper (II) oxide, 330-331 Copper (II) sulfate, 66 Copper sulfate, 66,260 Core electron An electron in an inner, complete level, 154... 

E.8 Copper metal can be extracted from a copper(II) sulfate solution by electrolysis (as described in Chapter 12). If 29.50 g of copper(II) sulfate pentahydrate, CuS04-511,0, is dissolved in 100. mL of water and all the copper is electroplated out, what mass of copper would be obtained ... 

E.26 Anhydrous copper(II) sulfate is difficult to dry completely. What mass of copper(II) sulfate would remain after removing 90% of the water from 250. g of CuS04-5H20 ... 

Suppose we were asked to prepare 250. mL of a solution that was approximately 0.0380 M CuS04(aq) from solid copper(II) sulfate pentahydrate, CuS04-5H20. What mass of the solid do we need ... 

Then, because the molar mass of copper(II) sulfate pentahydrate is 249.6 g-mol this amount of the pentahydrate corresponds to the following mass, t c.us04-5H2o ... 

We conclude that we should measure out about 2.37 g of copper(II) sulfate pentahydrate. In practice, we might find that we had spooned out 2.403 g, in which case the molarity would be 0.0385 M CuS04(aq). 

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