Nitrosophenylhydroxylamine

Experiment. — Nitrosophenylhydroxylamine.1 Phenylhydroxyl-amine (2-2 g.) is dissolved in 20 c.c. of N-hydrochloric acid and an aqueous solution of 1 -4 g. of sodium nitrite is rather quickly added with strong cooling in ice. White needles are at once precipitated. They are filtered with suction, washed with ice-cold water, and dried on porous plate. Melting point 59°. 

The substance is dissolved in ether and by passing in dry ammonia gas the ammonium salt is precipitated. From this salt the iron and copper salts, insoluble in water, are prepared by precipitation with Fe+ + + and Cu++ ( Cupferron ). 

In this reaction phenylhydroxylamine behaves like a secondary amine. To the class of nitrosohydroxylamines there belong also the so-called isonitramines and the compound of nitric oxide and potassium sulphite. 

The formation of the ammonium salt and the analytical application of nitrosophenylhydroxylamine as a reagent for the determination of iron and copper show that compounds of this kind are acidic. 

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Monomers like N-methylol acrylamide or N-methylol methacrylamide [1081] also have been suggested. Inhibitors can be phenol derivatives [1079] such as N-nitrosophenylhydroxylamine salt [1179]. 

Soon after the introduction of dimethylglyoxime as a specific reagent for nickel by Tschugaeff-Kraut-Brunck (1905-1907), Baudisch discovered a compound which precipitates copper and iron quantitatively from acid solutions.82 He appropriately named this reagent as cupferron . It is the water soluble ammonium salt of nitrosophenylhydroxylamine (5). When dissolved in chloroform, the whitish-grey copper compound gives a bright yellow solution and the brown yellow iron(III) compound a deep red solution. This behaviour reveals the inner complex character of these derivatives (6). 

During precipitation of metal cupferronates from mineral acid solutions, some nitrosophenylhydroxylamine is always coprecipitated. If attempts are made to wash out this water insoluble free acid with an organic solvent or ammonia, some metal is also lost and the remaining precipitate is often hydrolyzed. Consequently, cupferronates cannot be used as final weighing forms, and they serve only for purposes of precipitation and separation. These precipitates often have distinct colours which can form the basis of their estimation after extraction with suitable organic solvents.85... 

Figure 11.1 presents a scheme for the radioanalytical determination of 55Fe in water, biota, and sediment samples.11 This procedure is based on the separation of Fe from other metals (especially Cd, Cs, Cu, Ni, and Zn) on an anion exchange resin. The iron is then purified by coprecipitation with cupferron (the ammonium salt of nitrosophenylhydroxylamine). 

Different from the metallic nanoparticles, iron-oxide nanoparticles are chemically much more stable and readily synthesized. They can be prepared via high-temperature organic-phase decomposition of FeCup3, where Cup represents N-nitrosophenylhydroxylamine, C6H5N(N0)0 [30], decomposition ofFe(CO)s followed by oxidation [31-33], and decomposition of iron carboxylate [34, 35]. They can also be synthesized from partial reduce-tion/decomposition of Fe(acac)3 or Fe(acac)3 and M(acac)2 [36-38]. 

Cupferron reagent, the ammonium salt of nitrosophenylhydroxylamine, C6H5N(NO)ONH4. reddish-brown precipitate is formed in the presence of hydrochloric acid ... 

SYNS CUPFERRON N-HYDROXY-N-NITROSO-BENZENAMINE, AMMONIUM SALT KUPFERRON (CZECH) NCI-C03258 N-NITROSOFENYL-HYDROXYLAMIN AMONNY (CZECH) N-NITROSOPHENYLHYDROXYLAMIN AMMONIUM SALZ (GERMAN) N-NITROSOPHENYLHYDRO-XYLAMINE AMMONIUM SALT... 

NITROSOPHENYLHYDROXYLAMINE see AN0500 AMMONIUM OXALATE see ANO750 AMMONIUM PARAMOLYBDATE see ANM750 AMMONIUM PENTADECAFLUOROOCTANATE see ANP625... 

Q-1300,-1301. [WakoChem.USA] N-Nitrosophenylhydroxylamine salts analytical reagents, radical polymerization inhibitor, chelating agent, antioxidant, r ric. chemicals, germicides, fungicides. 

TETRACLORURO de ZIRCONIO (Spanish) (10026-11-6) Decomposes in the presence of moist air, forming a dense white cloud and hydrogen chloride fumes may ignite spontaneously. Reacts with water, steam, releasing heat, a dense white cloud, and hydrogen chloride. Violent reaction with bromine pentafluoride, lithium, oxygen difluoride, tetrahydrofuran. Contact with alkali metals may cause explosions. Incompatible with ammonium-V-nitrosophenylhydroxylamine. Attacks many plastics, rubber, and coatings. 

ZIRCAT (7440-67-7) Finely divided material is spontaneously flammable in air may ignite and continue to bum under water. Violent reactions with oxidizers, alkali hydroxides, alkali metals (and their compounds), carbon tetrachloride, cupric oxide, lead, lead oxide, lead peroxide (combined material can burn explosively, and is sensitive to friction and static electricity), nitryl fluoride, oxygen difluoride, phosphoms, potassium, potassium compounds (potassium chlorate, potassium nitrate), sodium borate, sodium hydroxide. Explodes if mixed with hydrated borax when heated. Contact with lithium chromate may cause explosion above 752°F/450°C. Forms explosive mixture with potassium chlorate. Dusts of zirconium ignite and explode in a carbon dioxide atmosphere. Contact with ammonium-V-nitrosophenylhydroxylamine above 104°F/40°C forms an explosive material. Incompatible with boron, carbon, nitrogen, halogens, lead, platinum, potassium nitrate. In case of fire, use approved Class D extinguishers or smothering quantities of dry sand, crushed limestone, clay. 

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