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Mercury II thiocyanate

Merkuri-jodid, n. mer curic iodide, mercury (II) iodide, -nitrat, n. mercuric nitrate, mercury-(II) nitrate. -oxyd, n. mercuric oxide, mercury (II) oxide, -rhodanid, n. mercuric thiocyanate, mercury(II) thiocyanate, -salz, n. mercuric salt, mercury (II) salt, -sulfati n. mercuric sulfate, mercury (II) sulfate, -sulfidt ti. mercuric sulfide, mercury (II) sulfide. -sulfozyamd, n. mercuric thiocyanate. [Pg.294]

Discussion. Potassium may be precipitated with excess of sodium tetraphenyl-borate solution as potassium tetraphenylborate. The excess of reagent is determined by titration with mercury(II) nitrate solution. The indicator consists of a mixture of iron(III) nitrate and dilute sodium thiocyanate solution. The end-point is revealed by the decolorisation of the iron(III)-thiocyanate complex due to the formation of the colourless mercury(II) thiocyanate. The reaction between mercury( II) nitrate and sodium tetraphenylborate under the experimental conditions used is not quite stoichiometric hence it is necessary to determine the volume in mL of Hg(N03)2 solution equivalent to 1 mL of a NaB(C6H5)4 solution. Halides must be absent. [Pg.359]

Mercury(II) thiocyanate method Discussion. This second procedure for the determination of trace amounts of chloride ion depends upon the displacement of thiocyanate ion from mercury(II) thiocyanate by chloride ion in the presence of iron(III) ion a highly coloured iron(III) thiocyanate complex is formed, and the intensity of its colour is proportional to the original chloride ion concentration ... [Pg.700]

Thiols react directly with non-activated alkynes [15] and with 1-alkynyl thioethers [16] to yield alkenyl thioethers in good yield (>76%), whereas thiocyanate anions only add to non-activated alkynes under acidic phase-transfer catalytic conditions on the addition of mercury(II) thiocyanate. Terminal alkynes are converted into vinyl thiocyanates, but disubstituted alkynes also form vinyl isothiocyanates [17]. Major by-products are the ketones formed by solvolysis of the alkynes. [Pg.147]

The solvent influences on the complex formation and stability have been reviewed by Golub et al.194 Several monomeric complexes of Hg(SCN)2 with N, O, P, As and S donor ligands are known with terminal Hg—SCN bonds.224-2 Some thiocyanate-bridged dimeric complexes of mercury(II) are also known.225,226 Recently the isolation of a mercury(II) thiocyanate complex with hexamethylenetetramine with exclusively N-bonded SCN groups has been published (Figure 9).233 The compounds (CH2)6N4-Hg(SCN)2 and (CH2)6N4-2Hg(SCN)2 exhibit covalently bonded Hg—s.394,595... [Pg.1063]

Mercury(II) perchlorate. 6 (or 4)dimethyl sulfoxide, 4073 Mercury(II) Af-perchlorylbenzylamide, 3644 Mercury(II) peroxybenzoate, 3630 Mercury(II) picrate, 3427 Mercury(II) sulfide, 4602 Mercury(II) thiocyanate, 0975 Mercury(I) nitrate, 4604 Mercury(I) oxide , 4608 Mercury(I) thionitrosylate, 4605 Mercury, 4595 Mercury nitride, 4610 Mercury peroxide, 4601 (9-MesitylenesuIfonylhydroxylami ne, 3164 Methacryloyl chloride, see 2-Methyl-2-propenoyl chloride, 1453 f Methanamine, see Methylamine, 0491... [Pg.2108]

Cadmium propionate, 2412 Calcium acetylide Methanol, 0582 Diazomethane Calcium sulfate, 0405 3,5-Dinitrotoluamide, 2936 Lithium tetrahydroaluminate Dioxane, 0075 Magnesium perchlorate, 4078 Magnesium Methanol, 4685 Mercury(II) thiocyanate, 0975 Silicon dioxide Hydrochloric acid, 4833 Sodium azide Heavy metals, 4753 Sodium Halocarbons (reference 10), 4790... [Pg.2318]

White precipitate of mercury (II) thiocyanate Blood red coloration due to complex formation Upon warming, red coloration is observed, with nitrogen oxide and hydrogen cyanide (caution toxic) being evolved Blue coloration due to complex ion formation... [Pg.535]

Chloride ions react with mercury (II) thiocyanate to form a sparingly dissociating mercuric chloride complex and liberate a stoichiometrically equivalent amount of thiocyanate ions (2CT + Hg(SCN)2 - Hgd2 + 2SCN) die thiocyanate reacts with iron (III) ions, yielding die intensely red ferric thiocyanate complex (SCN + Fe3+ -> Fe(SCN)2+), which is determined at 460 nm. [Pg.287]

Fluorides and mercury(II) ions bleach the colour because of the formation of the more stable hexafluoroferrate(III) [FeF6]3- complex and the non-dissociated mercury(II) thiocyanate species ... [Pg.248]

Mercury(II) nitrate solution white precipitate of mercury(II) thiocyanate Hg(SCN)2, readily soluble in excess of the thiocyanate solution. If the precipi-... [Pg.317]

DITHIOCYANATE MERCURY THIOCYANATE (DOT) MERCURY(II) THIOCYANATE THIOCYANIC ACID, MERCURY(2+) SALT... [Pg.871]

In the indirect thiocyanate method (not very sensitive, e 5 10 ) the determination of chloride [20-28] has been based on the displacement of SCN ion from the mercury(II) thiocyanate complex by chloride ions, to give a stable mercury chloride complex. After addition of Fe(III) in excess, the red Fe(SCN) complex is formed, and the absorbance is measured at 480 nm. In the FIA method the UV detection has been applied in the absence of Fe(III) ions [29]. [Pg.155]

Reagent. The carrier stream is prepared by dissolving 0.157 g of mercury (II) thiocyanate, 7.6 g of iron(III) nitrate, 0.8 mL of concentrated nitric acid, and 40 mL of methanol in water, maidng the final volume up to 250 mL. [Pg.790]

MERCURY(II) THIOCYANATE (592-85-8) Moderately unstable. Possible violent reaction with organic peroxides, peroxides, potassium chlorate, potassium iodate, silver nitrate, sodium chlorate, nitric acid. Incompatible with ammonia, chlorates, hydrozoic acid, methyl isocyanoacetate, nitrates, nitrites, perchlorates, sodium peroxyborate, trinitrobenzoic acid, urea nitrate. [Pg.744]

The manifold depicted in Fig. 5.13 Is used for the determination of chloride Ion In sea and tap water [31]. It uses a dialyser to remove interferents. The reagent Is a mixture of mercury(II) thiocyanate and Iron(III) nitrate, which, in the presence of the analyte, loses the red coloration of the Fe(IIl)-SCN- complex as a result of the formation of the stabler Hg(II)-CI-... [Pg.145]

Human activities have resulted in the release of a wide variety of both inorganic and organic forms of mercury. The electrical industry, chloro-alkali industry, and the burning of fossil fuels (coal, petroleum, etc.) release elemental mercury into the atmosphere. Metallic mercury has also been released directly to fresh water by chloro-alkali plants, and both phenylmer-cuiy and methylmercury compounds have been released into fresh and sea water -phenylmercury by the wood paper-pulp industry, particularly in Sweden, and methyl-mercury by chemical manufacturers in Japan. Important mercury compounds which also may be released into the environment include mercury(II) oxide, mercury(II) sulfide (cinnabar), mercury chlorides, mer-cury(II) bromide, mercury(II) iodine, mer-cury(II) cyanide, mercury(II) thiocyanate, mercury(II) acetate, mercury nitrates, mercury sulfates, mercury(II) amidochloride monoalkyl- and monoarylmercury(II) halides, borates and nitrates dialkylmercury compounds like dimethylmercury, alkoxyal-kylmercury compounds or diphenylmercury (Simon and Wiihl-Couturier 2002) (for quantities involved, see Section 17.4). [Pg.945]

See other pages where Mercury II thiocyanate is mentioned: [Pg.197]    [Pg.295]    [Pg.353]    [Pg.701]    [Pg.859]    [Pg.364]    [Pg.556]    [Pg.140]    [Pg.211]    [Pg.381]    [Pg.381]    [Pg.405]    [Pg.2328]    [Pg.2413]    [Pg.2422]    [Pg.357]    [Pg.300]    [Pg.2591]    [Pg.273]    [Pg.453]    [Pg.453]    [Pg.301]    [Pg.381]    [Pg.2025]    [Pg.2325]    [Pg.726]    [Pg.666]    [Pg.232]    [Pg.2590]    [Pg.15]   
See also in sourсe #XX -- [ Pg.1123 ]



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Mercury thiocyanate

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