Mercuric chlorid cyanid

Binary salts have varying hazards, one of which is toxicity. Some of the binary salts are highly toxic, such as sodium fluoride, calcium phosphide, and mercuric chloride. Cyanide salts are also highly toxic, such as sodium cyanide and potassium cyanide. The remaining salts, binary oxides, peroxide, hydroxides, and oxysalts are generally not considered toxic. 

Other ions, eg, ferrate, chloride, and formate, are determined by first removing the cyanide ion at ca pH 3.5 (methyl orange end point). Iron is titrated, using thioglycolic acid, and the optical density of the resulting pink solution is measured at 538 nm. Formate is oxidized by titration with mercuric chloride. The mercurous chloride produced is determined gravimetricaHy. Chloride ion is determined by a titration with 0.1 Ai silver nitrate. The end point is determined electrometricaHy. 

Merkuri-. mercuric, mercuri-, mercury(II). Merkuriah en, pi. Pharm.) mercurials. Merkuriahnittel, n. Pharm.) mercurial. Merkuri-ammoniumchlorid, n. mercuriammo-nium chloride, -azetat, n. mercuric acetate, mercury(II) acetate, -chlorid, n. mercuric chloride, mercury(II) chloride, -cyamd, n. mercuric cyanide, mercury(II) cyanide, -cyanwasserstoffs ure, /. mercuricyanic acid, cyanomercuric(II) acid. 

Cyanogen also may be prepared by the reaction of mercuric cyanide with mercuric chloride. Dry cyanogen gas may be obtained by this process ... 

Calcium Arsenate Calcium Phosphate Calcium Carbide Calcium Chlorate Calcium Chloride Calcium Chloride Calcium Chloride Calcium Chromate Calcium Chromate Calcium Chromate Calcium Cyanide Calcium Peroxide Calcium Fluoride Calcium Hydroxide Calcium Hypochlorite Calcium Phosphate Calcium, Metallic Calcium Nitrate Calcium Nitrate Calcium Oxide Calcium Peroxide Calcium Phosphate Calcium Phosphate Calcium Phosphide Calcium Resinate Calcium Resinate Calcium Resinate Calcium Phosphate Mercuric Chloride Mercurous Chloride... 

Mercaptosuccinic Acid, S-Ester with 0,0-Dimethyl Dithiophosphate Mercurialin Mercuric Acetate Mercuric Ammonium Chloride Mercuric Chloride Mercuric Chloride. Ammoniated Mercuric Cyanide Mercuric Iodide Mercuric Iodide, Red Mercuric Nitrate Mercubic Nitrate Monohydrate Mercuric Oxide... 

Compound Name Mercuric Chloride Mercuric Iodide Mercuric Chloride Mercuric Ammonium Chloride Mercuric Cyanide Mercuric Cyanide Mercuric Chloride Mercuric Nitrate Mercuric Oxide Mercuric Chloride Mercuric Nitrate Mercurous Chloride Mercurous Nitrate Mercurous Chloride Mesityl Oxide Calcium Resinate Methyl Methacrylate N-Butyl Methacrylate Glycidyl Methacrylate Ethyl Methacrylate Methyl Methacrylate Methallyl Chloride Methallyl Chloride Formaldehyde Solution Methane... 

L. Berczeller has shown that the presence of acids, chlorides, bromides, iodides, thiocyanates, and morphine accelerate the reaction while the presence of tartrates, sulphates, oxalates, carbonates, mercuric chloride, bromide, iodide, and cyanide, most alkaloids, colloids, proteins, etc., inhibit the reaction. Hydrocyanic acid, unlike other acids, also inhibits the reaction. A. Skrabal has shown that Landolt s reaction has a temp, coeff. greater than unity, so that the velocity of the reaction increases with a rise of temp. but if the system contains an excess of sodium sulphate, the temp, coeff. is less than unity, and the velocity of the reaction decreases with a rise of temp. 

Mercury fulminate is relatively resistant to the action of dilute acids, in particular to that of nitric acid, but concentrated acids cause decomposition. Thus, under the influence of nitric acid decomposition occurs with evolution of NO, CO, acetic acid and mercuric nitrate. Under the influence of concentrated hydrochloric acid free fulminic acid is evolved (with an odour resembling that of hydrogen cyanide) as well as the decomposition products hydroxylamine hydrochloride, formic acid, mercuric chloride (Carstanjen and Ehrenberg [32] Scholl [33]). Mercury fulminate explodes on direct contact with concentrated sulphuric acid. 

In anodic dissolution of mercury in a solution of nitric acid, where both mercurous and mercuric salts are asumed to be completely dissociated, both the formed ions enter the solution in the ratio of their respective activities hKo+/ h1 ++ = 76. When alkali cyanide is used as electrolyte the bivalent ions formed on dissolution are predominantly consumed for the formation of the complex Hg(CN). As a result of the formation of this complex the concentration of free Hg++ jpns decreases considerably in accordance with the neghgible degree of dissociation of the above-mentioned complex, and consequently the dissolution potential of the system Hg/Hgt+ also decreases. For this reason, mercuric ions converted to mercuricyanide complex can be considered to be practically the sole product of the anodic process while the amount of univalent mercury ions is quite negligible. Contrary to this, on dissolving mercury in a solution of hydrochloric acid mercurous ions are predominantly formed due to the slight dissociation of mercurous chloride, the main product of the reaction. 

A similar consideration can be applied to the cathodic processes. In a solution of mercuric nitrate bivalent mercury will bo reduced to univalent until the ratio of the respective activity of the mercurous salt formed and tho mercuric salt still remaining reaches the equilibrium value. During the course of further reaction the ratio of activities of both ions in the solution will not change any longer, and metallic mercury will be deposited. Therefrom, it is evident that mercuric nitrate cannot be quantitatively reduced to mercurous salt. Bivalent mercury can be reduced practically completely to univalent in the case of mercuric chloride. As the solubility of the mercurous chloride formed by the reduction and consequently also the concentration of Hg2+ ion is very small the equilibrium between the ions in the solution will be attained only then, when nearly all Hg++ ions will be reduced to univalent ones. On the other hand on reduction of the very slightly dissociated cyanide complex Hg(CN) the equilibrium between mercurous and mercuric ions is reached at the very beginning of electrolysis as soon as a hardly noticeable amount of Hg++ ions has been formed from that moment on metallic mercury will be deposited at the cathode with practically 100 p. o. yield. 

Colloidal platinum still further resembles organic ferments in its action upon hydrogen peroxide in that its activity is reduced or partially paralysed by the addition of poisons such as hydrogen cyanide, hydrogen sulphide, or mercuric chloride. After a time, however, the metal may recover from these. 

Mauricheau-Beaupre 4 has shown that treatment of aluminium filings with a small proportion of mercuric chloride and potassium cyanide yields a powder stable in dry air. He called this substance hydrogenite, and found that one kilogram of it treated with water yields 1300 litres of pure hydrogen, measured at 15° C. and 760 mm. 

Cyclopentadiene reacts with mercuric cyanide in aqueous solution, giving the insoluble cream compound CsHsHgCN. Like the corresponding iodide (which is also cream) this compound is fairly stable in air, but does not melt sharply (62). By the reaction of indenyl lithium and mercuric chloride in dry ether, indenyl mercuric bromide (the bromine being... 

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