Tris 1-hydrate

Metal carboxvlates M(OOCR)x Ba(OOCCH3)2, Barium acetate tri-hydrate... 

T) mit Hexamel hylsilazan358 4,67 g (29 mmol) Hexamethylsilizan, 16mmol 1,2-Diacyl-hydrazin und 5,04 g (16 mmol) Tetrabutylammonium-fluorid-Tris-hydrat erhitzt man 21 -48 h unter Stiekstoff zum Sie-den. Nach Destination oder durch Umkristallisation erhalt man die 2,5-disubstituierten 1,3,4-Oxadiazole Ausbeute 63-81%. 

Kupfernitral/Ton (,daycop )s- -2 Ineinem l-/-Kolben werden26 g Kupfer(II)-nilrat-Tris-hydrat und... 

The structures of zinc aspartate tri-hydrate, urea phosphate and cycloserine hydrochloride have been determined by 3-dimensional x-ray methods ami refined by IBM 704 least-squares computations The zinc aspartate analysis [14] reveals H positions and H-bonding which leads to a ring structure for the aspartate ion. Urea phosphate shows strong H-bond throughout the structure [15]. Seven H s are available for nine short bonds. Cycloserine hydrochloride [16, 17] shows seven short mtermolecular distances, suggesting 0—H O,... 

Anhydrous ruthenium(lll) chloride, RuCL, is made by direct chlorination of the metal at 700°C. Two aliotropic forms result. The trihydrate is made by evaporating an HQ solution of rulheinuiu(III) hydroxide to dryness or reducing ruthenium(VIII) oxide in a HQ solution. The tnhydrate, RuCk 3R>0, is the usual commercial form. Aqueous solutions of the tri-hydrate are a straw color in dilute solution and red-brown in concentrated solution. Ruthenium(lll) chloride in solution apparently forms a variety of aquo- and hydroxy complexes. The analogous bromide. RuBr3, is made by the same solution techniques as the chloride, using HBr instead of HQ. 

Sodium Chlorite, NaC102, wh crysts, exists in anhyd tri-hydrated forms, mp 175 200° (decomp, temp dependent upon moisture content). The solubility of NaC102 is reported by Taylor et al(Ref 1). Commercial production of NaC102 in the US is based upon the reduction of Ca(C103)2 by HC1. The chlorate is reduced to chlorine dioxide, and the hydrochloric acid is oxidized to chlorine ... 

Iron metaniobates(iv) with structures of the natural minerals, ilmenite and pseudo-brookite have been prepared by direct reaction of the oxides under vacuum at 1000—1100°C. The compounds are stable in air up to 500°C, but are oxidized at higher temperatures.326 a-Sr3Fe07 x has been found to be isostructural with Sr3Ti07.327 Synthesis and thermal decomposition of iron(m) normal selenite mono-or tri-hydrate, Fe203,3Se02,xH20 (x = 1 or 3) have been reported.328... 

Natrium-dipropyl-dithiophosphinat-Tris-hydrat 152 85"/0 Schmp. 50-51°... 

Tri-hydrates of acetic acid HAc- (H20)3 and the most stable six-membered ring... 

Interaction of the corresponding rhodium chloride with water and silver triflate gives the tris hydrate ... 

Heptan 1-Amino-1-hydroxy- -Tris-hydrat E14a/2, 10... 

The dihydrate is formed by evaporation at ordinary temperature of an ethereal solution of the hexahydrate which has been dried with calcium nitrate or by crystallisation of the hexahydrate from concentrated nitric acid solution. It yields small lustrous plates, thick and square, probably rhombic, and possessing a green fluorescence. It melts at 179-3° C. It is much more stable than the trihydrate, and can be kept in a vacuum desiccator with caustic alkali or i hosphorus pentoxide without any loss of water. It dissolves readily in ether. If the dihydrate is heated in a current of carbon dio.xide at 98° C. a product corresponding very nearly in composition to the nioiiohydrate, U03(N03)3.H20, is obtained at 160° C. under the same conditions the ankydi ffus salt, U02(N03)2, is obtained. The latter may also be obtained by passing a current of dry nitric anhydride over the tri-hydrate carefully heated at 170° to 180° C. It is a yellow amorphous powder, readily soluble in water with c -olution of heat. It reacts violently with ether. When heated to 200° C. it decomposes and leaves a mixture of uranic acid, UO3.H2O, and uranic anhydride. ... 

Density functional theory (DFT) has emerged as a powerful technique for the solution of the Schrodinger equation at affordable computational costs. Several groups have used DFT to address the effect of electron correlation in ion-water systems. Combariza and Kestner studied short-range interactions and charge transfer in mono and tri-hydrates of Li", Na", F, and CF. The accuracy of their DFT predictions was assessed by comparing electron affinity and atomic polarizability to experimental values. Small water and ion-water clusters were also analyzed and compared to those predicted by effective potentials in MD simulations. 

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