II Sulfate

Copper(II) sulfate (KOPP-er two SUL-fate) is a white crystalline powder in its anhydrous state, although it occurs most commonly as the pentahydrate, CuS04 5H20, which is a blue granular crystalline solid. When the pentahydrate is heated, it loses its water of hydration and returns to its white, powdery anhydrous state. The transition between its white anhydrous form and its blue hydrated form is sometimes used in devices and toys that indicate the presence or absence of moisture in the air. 

Copper(II) sulfate is probably the most important and most widely used of all copper compounds. It is used in agriculture, the paints and covering industry, in electrical applications, in the production of other chemicals, and in other industrial and commercial applications. 

Copper(II) sulfate occurs in nature as the mineral cal-canthite. Calcanthite is somewhat rare since copper(II) 

Copper(H) sulfate pentahydrate. Red atoms are oxygen yellow atom is sulfur and turquoise atom is copper. Gray sticks are double bonds. 

1 Copper(ll) sulfate gets the is made from sulfuric acid, 

Hydroboration of 1-bromo-l-alkynes with chloro(thexyl)-borane leads to the synthesis of alkynyl ketones in 61-63% yields by the sequence of reactions shown in eq 5. Sequential treatment of alkenylchloro(thexyl)boranes, which are formed by the reaction of chloro(thexyl)borane with alkynes, with lithium chloro-propargylide and aldehydes affords 1,3-enynols or 1,2,4-trienols depending on the reaction conditions.  

Reductive Cyclization of ( -Azidoalkenes. Hydroboration of -azidoalkenes with chloro(thexyl)borane followed by hydrolysis affords, via an intramolecular reductive cyclization, the corresponding p)UTolidine (78%) or the piperidine (53%) (eq 7).  

Kramer, G. W. Levy, A. Midland, M. M. Organic Syntheses via Boranes, Wiley New York, 1975 Chapter 9. 

Alkylchloro(thexyl)boranes prepared from terminal alkenes can be hydrolyzed with one equivalent of water and then oxidized with pyridinium chlorochromate (PCC) to the corresponding aldehyde in moderate yields (eq 6).  

Reduction of Carboxylic Acids to Aldehydes. Aliphatic carboxylic acids are reduced rapidly (15 min) and aromatic carboxylic acids are reduced slowly (24 h) by chloro(thexyl)borane- 

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In general ketones are more stable than their enol precursors and are the products actually isolated when alkynes undergo acid catalyzed hydration The standard method for alkyne hydration employs aqueous sulfuric acid as the reaction medium and mer cury(II) sulfate or mercury(II) oxide as a catalyst... 

When 2 heptyne was treated with aqueous sulfunc acid containing mercury(II) sulfate two products each having the molecular formula C7H14O were obtained in approximately equal amounts What are these two compounds ... 

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). 

Sellaite, see Magnesium fluoride Senarmontite, see Antimony(III) oxide Siderite, see Iron(II) carbonate Siderotil, see Iron(II) sulfate 5-water Silica, see Silicon dioxide Silicotungstic acid, see Silicon oxide—tungsten oxide—water (1/12/26)... 

Sylvite, see Potassium chloride Szmikite, see Manganese(II) sulfate hydrate... 

Tris( 1,10-phenanthroline)-iron(II) sulfate 1.06 (I.OOMH2SO4) Red to faint blue... 

Manganese(II) can be titrated directly to Mn(III) using hexacyanoferrate(III) as the oxidant. Alternatively, Mn(III), prepared by oxidation of the Mn(II)-EDTA complex with lead dioxide, can be determined by titration with standard iron(II) sulfate. 

Standard Manganese(ll) Solution. Dissolve exactly 16.901 g ACS reagent grade manganese(II) sulfate hydrate in water and dilute to 1 E. 

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

Methylpyridine Hydrogen peroxide, iron(II) sulfate, sulfuric acid... 

Tetrasodium hexakiscyanoferrate decahydrate [14434-22-1], Na4[Fe(CN)g] IOH2O, or yellow pmssiate of soda, forms yellow monoclinic crystals that are soluble in water but insoluble in alcohol. It is slightly efflorescent at room temperature, but the anhydrous material, tetrasodium hexakiscyanoferrate [13601 -19-9], Na4[Fe(CN)J, is obtained at 100°C. The decahydrate is produced from calcium cyanide, iron(II) sulfate, and sodium carbonate in a process similar to that for the production of K4[Fe(CN)g] 3H2O. It is used in the manufacture of trisodium hexakiscyanoferrate, black and blue dyes, as a metal surface coating, and in photographic processing. 

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