Iodide Mercurous chloride

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... 

Mercuric Chloride Mercuric Iodide Mercuric Chloride Mercuric Ammonium Chloride... 

Many mercury compounds are labile and easily decomposed by light, heat, and reducing agents. In the presence of organic compounds of weak reducing activity, such as amines (qv), aldehydes (qv), and ketones (qv), compounds of lower oxidation state and mercury metal are often formed. Only a few mercury compounds, eg, mercuric bromide/77< 5 7-/7, mercurous chloride, mercuric s A ide[1344-48-5] and mercurous iodide [15385-57-6] are volatile and capable of purification by sublimation. This innate lack of stabiUty in mercury compounds makes the recovery of mercury from various wastes that accumulate with the production of compounds of economic and commercial importance relatively easy (see Recycling). 

Mercuric chloride is widely used for the preparation of red and yellow mercuric oxide, ammoniated mercury/7(9/USP, mercuric iodide, and as an intermediate in organic synthesis. It has been used as a component of agricultural fungicides. It is used in conjunction with sodium chloride in photography (qv) and in batteries (qv), and has some medicinal uses as an antiseptic. 

No turbidity with alkaline mercuric chloride—potassium iodide reagent USP test. 

Nicotine may be detected by the colourless, crystalline mercurichloride obtained when an aqueous solution is added to a solution of mercuric chloride, by the black precipitate formed under similar conditions with potassium platinic iodide and the characteristic crystalline periodide, BI2. HI, m.p. 123°, produced on admixture, under specified conditions, 2 of ethereal solutions of nicotine and iodine (cf Anabasine, p. 43). A polarographic study of nicotine has been made by Kirkpatrick. ... 

Merkuro-. mercurous, mercury (I), -azetat, n. mercurous acetate. mercury(I) acetate, -chlorld, n. mercurous chloride, mercury(I) choride. -chrom, n. (Pharm.) mercuro chrome, -jodid, n. n ercurous iodide, mer-cury(I) iodide. -nitrat, n. mercurous nitrate, mercury(I) nitrste. -oxyd, n. mercurous oxide, mercury(I) oxide, -salz, n. mercurous salt, mercury (I) salt, -sulfat, n. mercurouasulfate, mercury(I) sulfate, -sulfid, n. mercurous sulfide, mercury(I) sulfide, -verbindung, /. mercurous compound, mercury (I) compound. 

The reactions of mercuric iodide, mercuric bromide, and mercuric chloride with the excited species produced in the hexafluoroethane plasma were examined first, as the expected products were known to be stable and had been well characterized 13). Thus, these reactions constituted a "calibration of the system. Bis(trifluoromethyl)mercury was obtained from the reaction of all of the mercuric halides, but the highest yield (95%, based on the amount of metal halide consumed) was obtained with mercuric iodide. The mole ratios of bis(trifluoro-methyDmercury to (trifluoromethyl)mercuric halides formed by the respective halides is presented in Table I, along with the weight in grams of the trifluoromethyl mercurials recovered from a typical, five-hour run. 

Determination of the Iodine Value.—Pure iodine (2-5 g.) and mercuric chloride (3 g.) are each dissolved in 50 c.c. of pure spirit and the clear solutions are mixed. After twelve hours the iodine titre of the mixture is determined in a 10 c.c. portion by adding 10 c.c. of 10 per cent potassium iodide solution and titrating with 0-1 IV-thiosulphate solution. 

Most alkaloids are isolated from plant extracts by conversion into the difficultly soluble salts which they form with complex acids such as hexachloroplatinic acid, chlorauric add, phosphotungstic add, hydroferro-cyanic add, Rdnecke s add, etc. Perchloric add, picric add, flavianic add, mercuric chloride, iodine in potassium iodide are also used. 

Dobbin s reagent analychem A mercuric chloride-potassium iodide reagent used to test for caustic alkalies in soap. dab-anz re a- ant ... 

It has been found on examination of the ammino-derivatives of mercuric halides that the nature of the halogen present has a marked effect on the stability ol the compound. Thus, diammino-mercuric chloride, [Hg(NH3)2]Cl2, is stable and does not readily lose ammonia, whereas the corresponding iodide, diammino-mercuric iodide, [ITg (NH3) JI2, readily loses ammonia at ordinary temperature. The stability decreases in the order chloride, bromide, iodide. 

Many derivatives of this series of salts have been prepared. For example, the chloride, if freshly prepared, yields in aqueous solution crystalline salts with chloroplatinic aeid, potassium iodide, and mercuric chloride,1 and numerous acido-derivatives have been prepared. 

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... 

Silver foil is transformed by an aq. soln. of the trichloride into silver chloride and iodide silver oxide with an excess of the trichloride is transformed into the chloride and iodic acid with more silver oxide, silver iodate is formed and with an excess of the oxide and a boiling soln. some silver periodate is formed. Mercuric oxide is slowly transformed into mercuric chloride and oxide chlorine, oxygen, and possibly chlorine monoxide are evolved. Aq. soln. of the trichloride give a precipitate of iodine with a little stannous chloride with more stannous chloride, some stannous iodide is formed. Consequently, although chloroform extracts no iodine from the aq. soln., it will do so after the addition of stannous chloride. Sulphur dioxide and ferrous sulphate are oxidized. 

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. 

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