Mercurous ferricyanide

Mercuric ferricyanide, Hg3[Fe(CN)6]2, may be obtained by adding a concentrated aqueous solution of potassium ferricyanide to a solution of mercuric chloride in alcohol and ether. The precipitate is bright yellow in colour, and fairly stable when dry.5... 

Mercurous ferricyanide, Hg3[Fe(CN)6], is obtained as aflocculent cream-coloured precipitate on the addition of mercurous nitrate to potassium ferricyanide solution.5 It turns blue on exposure to air. 

A -Piperideine-N-oxide was obtained along with a dimeric product by oxidation of N-hydroxypiperidines with mercuric acetate or potassium ferricyanide (107-109). 2l -Pyrroline-N-oxide is formed by oxidation of N-ethylpyrrolidine with hydrogen peroxide with simultaneous formation of ethylene (110). 

Chemical complexes of various transition metals have been shown to promote N-nitrosation (28). These metal complexes include ferrocyanide, ferricyanide, cupric ion, molybate ion, cobalt species, and mercuric acetate. All of the reactions are thought to proceed by oxidation-reduction mechanisms. However, such promotion may not be characteristic of transition metal complexes in general, since ferricyanide ion has been shown to promote nitrosation in metalworking fluids, whereas ferric EDTA does not (2 0). Since the metalworking operation generates metal chips and fines which build up in the fluids, this reaction could be of significance in the promotion of nitrosamine formation in water-based metalworking fluids. 

Fire or explosion hazard may arise from the foUowing ammonia reactions Reaction with halogens produces nitrogen trihahdes which explode on heating its mixture with fluorine bursts into flame reacts with gold, silver, or mercury to form unstable fulminate-type shock-sensitive compounds similarly, shock-sensitive nitrides are formed when ammonia reacts with sulfur or certain metal chlorides, such as mercuric, or silver chloride liquid ammonia reacts violently with alkah metal chlorates and ferricyanides. 

Potassium Chlorate. .. Potassium Triiodo Mercurate(ll) Potassium Chloride Potassium Chlorate Potassium Chromate Potassium Cyanide Potassium Dichromate Potassium Ferricyanide Potassium Ferrocyanide Potassium Fluoride Potassium Formate Potassium Hydride Potassium Hydrogen Phthalate Potassium Hydroxide Potassium lodate... 

With certain compounds, such as pyrazoline carboxylic acids and esters, potassium ferricyanide or silver nitrate has been used,509 and for those compounds unsubstituted on nitrogen, mercuric oxide or acetate.76 Lead dioxide has been successful for the oxidation of 1-alkyl-and 1-arylpyrazolines,9i 76,83 and in certain instances even chromic acid, but not hydrogen peroxide or silver oxide.76 See also L. Smith521 and Birkinshaw et al.b22... 

Occluded hydrogen is more reactive chemically than the normal gas. Hydrogenated palladium precipitates mercury and mercurous chloride from an aqueous solution of the dichloride, without any evolution of hydrogen. It reduces ferric salts to ferrous potassium ferricyanide to ferrocyanide chlorine water to hydrochloric add iodine water to hydriodic acid 2 chromates to chromic salts ceric to cerous salts whilst cupric, stannic, arsenic, manganic, vanadic, and molybdic compounds are also partially reduced.3... 

As already oudined, inhibition is essentially complete when caused by reagents that react with sulfhydryl groups (for example, p-chloro-mercuribenzoate, p-mercuribenzoate, o-iodosobenzoate, L-ascorbic acid silver, cupric, and mercuric ions iodine, and ferricyanide) this inactivation can be reversed to some extent by hydrogen sulfide and by cysteine. Lineweaver—Burk graphs have shown that the action of L-ascorbic acid is noncompetitive, and L-ascorbic acid acting in the presence of cupric ions probably causes formation of an inactive cuprous-enzyme. The action of p-chloromercuribenzoate on barley beta-amylase has been shown to be a competitive inhibition. In contrast, the soya-bean p-chloromercuribenzoate inhibition is noncompetitive, and the extent of inhibition is inversely related to the concentration of acetate ion. The latter exhibits a protective effect, and there... 

Mercuric oxide, HgO, is formed as a yellow precipitate by adding a base to a solution of mercuric nitrate or as a red powder by heating dry mercuric nitrate or, slowly, by heating mercury in air. The yellow and red forms seem to differ only in grain size it is a common phenomenon that red crystals (such as potassium dichromate or potassium ferricyanide) form a yellow powder when they are ground up. Mercuric oxide liberates oxygen when it is strongly heated. 

Potassium permanganate. Dimethyl sulfide-Chlorine. Dimethyl sulfoxide. Dimethyl sulfoxide-Chlorine. Dimethylsulf-oxide Sulfur trioxide. Dipyridine chro-mium(VI) oxide. Iodine. Iodine-Potassium iodide. Iodine tris(trifluoroacetate). Iodosobenzene diacetate. Isoamyl nitrite. Lead tetraacetate. Manganese dioxide. Mercuric acetate. Mercuric oxide. Osmium tetroxide—Potassium chlorate. Ozone. Periodic acid. Pertrifluoroacetic acid. Potassium ferrate. Potassium ferricyanide. Potassium nitrosodisulfonate. Ruthenium tetroxide. Selenium dioxide. Silver carbonate. Silver carbonate-Celite. Silver nitrate. Silver oxide. Silver(II) oxide. Sodium hypochlorite. Sulfur trioxide. Thalli-um(III) nitrate. Thallium sulfate. Thalli-um(III) trifluoroacetate. Triphenyl phosphite ozonide. Triphenylphosphine dibromide. Trityl fluoroborate. 

Diimide, HN=NH. The reagent, generated in situ by cupric ion-catalyzed oxidation of hydrazine with oxygen (air), hydrogen peroxide, potassium ferricyanide, or mercuric oxide, reduces olefins, alkynes, and azo compounds. Reduction of the... 

Several methods can be used for the determination of chloride in water [2], The argentometric and mercuric nitrate methods are based on the titration of chlorine in the presence of an indicator. Experimental procedures are easy, but many substances may interfere with the results. There are also other methods such as potentiometry, capillary electrophoresis and other automated methods (ferricyanide method or flow injection analysis). 

Ferric chloride Acridines from acridanes s. 1, 23, 756 2, 91/2 Potassium ferricyanide, mercuric oxide Suhst. oximes from subst. hydroxylamines s. 3, 403 FeCl,... 

Irioxide, platinum, silver, potassium chlorate, potassium ferricyanide, potassium mercuric cyanide, silver chloride, stibine, tellurium halides, tellurium hydropentachloride, tetramethy-lammonium amide, trimethylammonium amide, trioxygen difluoride, vinyl acetate. Violent polymerization with ethylene oxide. Attacks some coatings, plastics, and rubber. Attacks copper, brass, bronze, aluminum, steel, and their alloys. 

Ferricyanide ions are demasked in analogous fashion by mercuric chloride and iron+ ions are set free. However, this does not detract from the detection of ferrocyanide because a,ct -dip5n idyl reacts only with iron+ ions. 

Thiocyanates and/or iodides interfere with the sensitive Pmssian blue test for ferrocyanides when carried out in a micro test tube or on a spot plate. There is simultaneous formation of red ferrithiocyanate or free iodine, which interfere with the decisive detection of small amounts of Prussian blue. If, however, the test is carried out on filter paper impregnated with ferric chloride, no difficulty is experienced because of thiocyanates or iodides. A capillary separation succeeds through the fact that ferric thiocyanate is readily decomposed by mercuric chloride, sodium fluoride, or sodium thiosulfate. If there is danger of interference by ferricyanide, the second procedure should be followed. 

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