Hydrazine acid-base properties

The u.v. and i.r. spectra of NH3 and Cl2 codeposited in a N2 matrix at 20 K are consistent with the formation of a charge-transfer complex between these molecules.21 The formation of chloramine in high yield from Cl2 and NH3 in the presence of a ketone has been reported.22 Gas-phase as well as gas-liquid-phase reactions were investigated to assess the suitability of this reaction for the production of hydrazine. However, from a study of the acid-base properties of Br2 in liquid NH3 it has been deduced that BrNH2 does not exist in dilute solutions at low temperatures, owing to the stability of the solvated Br+ species.23... 

Anhydrous copper(II) sulfate, 7 773 Anhydrous ethanol, production by azeotropic extraction, 8 809, 817 Anhydrous gaseous hydrogen sulfide, 23 633 Anhydrous hydrazine, 13 562, 585 acid-base reactions of, 13 567-568 explosive limits of, 13 566t formation of, 13 579 vapor pressures of, 13 564 Anhydrous hydrogen chloride, 13 809-813 physical and thermodynamic properties of, 13 809-813 purification of, 13 824-825 reactions of, 13 818-821 uses for, 13 833-834... 

This hydrogen transfer is essentially an intramolecular acid-base reaction. The hydrogen of the coordinated alcohol function is acidified by coordination to the copper center whilst the hydrazine ligand possesses basic properties. The elimination of the hydrazine substituent is irreversible under these neutral conditions. Indeed, in the absence of excess base, DBADH2 is unable to displace the alkoxide ligand from the copper complex G. 

The chemical properties o orthophosphoric add.—W. Muller-Erzbach21 has discussed the affinity of the metals for phosphoric acid. J. Thomsen found the avidity of a mol. of phosphoric acid for one of sodium hydroxide to be a quarter of the value of that for hydrochloric acid. The affinity of phosphoric acid for the bases is greater than that of carbonic acid, boric acid, phosphorous acid, and hypophosphorous acid. The catalytic action of phosphoric acid on the reaction between bromic and hydriodic acids has been studied by W. Ostwald on the reaction between iodic and sulphurous acids, by R. Hopke and A. Purgotti and L. Zanichelli on hydrazine sulphate, N2H4.H2S04. According to W. Ostwald, the velocity constant for the inversion of cane sugar by phosphoric acid is 6-21 when the value for hydrochloric acid is 100 and J. Spohr showed that the presence of neutral salts at 25° retards, or at 40° completely suppresses,the activity of phosphoric acid. 

Thioacetamide, which is well established for the precipitation of ZnS in solutions, can be also used [68] in which case the films have been deposited from acidic solutions. The addition of urea has a beneficial effect on the adherence [68], Some attempts have been made to deposit ZnS by using thiosulfate-based solutions [16], As compared to CdS and PbS it appears that the deposition of ZnS films is not yet optimized and in addition presents some differences in the growth mechanism. This is illustrated by the lower activation energy values ( 20 kJ.rnol" ) which has been determined in the ammonia-thiourea-hydrazine process, which is more likely characteristic of a diffusion limited growth [69]. The deposition of indium sulfide has been also reported in acidic solutions using TA [52], along with a detailed study of the influence of the deposition conditions on the structural and optical properties of the films. 

Properties and reactions of nitramines Secondary nitramines are neutral, primary nitramines form salts with bases, but an excess of alkali often causes decomposition to the carbonyl compound, nitrogen, and water. Secondary nitramines and aqueous alkali afford nitrous acid, aldehyde, and primary amine. Acids decompose primary aliphatic nitramines with formation of nitrous oxide in a reaction that has not yet been clarified thus these compounds cannot be hydrolysed by acid to amines in the same way as nitrosamines, although, like the latter, they can be reduced to hydrazines. Primary and secondary aromatic nitramines readily rearrange to C-nitroarylamines in acid solution. Most nitramines decompose explosively when heated, but the lower aliphatic secondary nitramines can be distilled in a vacuum. 

CHEMICAL PROPERTIES stable under ordinary conditions of use and storage hazardous polymerization has not been reported can react with strong bases, strong acids, alcohols, hydrazine, and combustible, organic or other easily oxidized materials FP (unknown) LFL/UFL (unknown) AT (unknown). 

In the case of peraksine [RP-5 (27)] it was shown to have the formula C19H22N2O2, a fact not readily derived from combustion analysis since the free base crystallized from alcohol in a hydrated form (27). It has also been observed that this water of solvation could be displaced by chloroform (20). Peraksine has UV-absorption typical of a 2,3-disub-stituted indole and reacted with benzoyl chloride to form an 0-benzoyl derivative. The second oxygen was apparently present as a cyclic ether when it was found that although peraksine did not react with hydrazine derivatives, it was reducible with sodium borohydride to furnish a diol (mp 290°-291° [a]j) - -41° in Py diacetate, mp 103°-105°). This diol readily lost the elements of water upon acid treatment to afford a new ether, deoxyperaksine, 230° change in crystalline form (mp 255°-257°). Because of these properties peraksine was considered to possess a cyclic hemiacetal moiety. 

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