Mercury complexes basic salts

The weak base HgO can be dissolved in weak acids to form mercury(II) salts. Usually an excess of the acid is necessary to prevent hydrolysis and the formation of basic salts. The complex formation between mercury(II) and carbonate has been studied.277 Three complexes were found, the simplest formulations being as shown in equations (12)-(14). 

P. C. Ray and 8. C. Mukherjee found the degree of ionization to be 0-11 for a mol of the salt in 32 litres. P. C. Ray and N. Dhar found that if the aq. soln. be kept in a closed vessel for some time, some of the mercuric nitrite forms mercurous nitrate and a basic salt is formed thus in 3 weeks, a soln. of sp. gr. 1-065 contained mercuric mercurous mercury as 13-7 1. P. C. Ray and N. Dhar found that the conductivity measurements of aq. soln. of mercurous nitrite agree with the assumption that a complex Hg2(N02) 5-ion is present this corresponds with mercurosic nitrite, HgN02.2Hg(N02)2. For a dilution v=187, A—62-33, and when c=561, A=80-10. With dil. soln., hydrolysis occurs. If the aq. soln. be sealed up in an... 

Complexes with carboxylates and related ligands Complexes with inorganic oxo anions Basic salts of mercury (II)... 

Heavy metals are widely used as catalysts in the manufacture of anthraquinonoid dyes. Mercury is used when sulphonating anthraquinones and copper when reacting arylamines with bromoanthraquinones. Much effort has been devoted to minimising the trace metal content of such colorants and in effluents from dyemaking plants. Metal salts are used as reactants in dye synthesis, particularly in the ranges of premetallised acid, direct or reactive dyes, which usually contain copper, chromium, nickel or cobalt. These structures are described in detail in Chapter 5, where the implications in terms of environmental problems are also discussed. Certain basic dyes and stabilised azoic diazo components (Fast Salts) are marketed in the form of tetrachlorozincate complex salts. The environmental impact of the heavy metal salts used in dye application processes is dealt with in Volume 2. 

By comparison with the mercury(I) and mercury(II) ions (Chapter 56.1), the coordination chemistry of (10) and (11) has received little attention. Both ions disproportionate to Hg° and Hg2+ /Hg2+ in media more basic than those from which they can be prepared. However, the existence of (11) (which can be regarded as a complex of (10) with Hg°) and the cation-anion coordination found in solid salts of (10)38 suggest that this ion, at least, might form stable complexes with suitable weak donors. In addition, the formation of as yet incompletely characterized Hg2BrCI04 2SnBr2, which may contain both Hg—Hg and Hg—Sn bonds,42 and the isolation and characterization of [ (np3)Co HgHg Co(np3) ] (1 see Section 11.2) may presage a wider occurrence of catenated heterometallic polymercury species. Slow disproportionation of (11) into (10) and Hg3-X(MF6) occurs even in liquid S02.39 As discussed below, there is evidence for mercury atom transfer between (10) and (11) in liquid S02. 

When ethylene was passed into a basic solution of Hg(OAc)2 containing a catalytic amount of [Rh2(OH)3(C5Me5)2]+, ethanol was formed.617 It appears that mercury salts of the type HOCH2CH2HgOAc are formed in a stoichiometric reaction so that this is not strictly a catalytic activation of ethylene by the rhodium complex. 

The base-catalyzed conversion of 5-alkyl-substituted isothiazolium salts 88 (R = Me, R = Et) to 2,3-dihydrothio-phene derivatives 329 occurs in basic conditions via intermediates 328. The distribution of diastereomers 329 is dependent on the base and aryl substituent <1997SUL35>. Similar behavior was observed in the case of 88 (R = R =-(0112)4-) <1996JPG424>. The condensation of 5-Me-substituted isothiazolium salts 88 with a second molecule of a different isothiazolium salts affords haA -thia-Eh-diazapentalenes 330. In this way, macrocyclic ethers 332 were prepared from 331 and their complexation behavior toward sodium(l), silver(l), and mercury(n) studied <2001PS(170)29>. 

Since protamine is strongly basic, it forms salt-like complexes with various inorganic and organic acids. The sulfate, hydrochloride, nitrate, phosphate, and acetate salts are soluble in water, but the picrate, flavianate, and phosphotungstate salts are almost insoluble in water. Protamines also form scarcely soluble salts with silver nitrate, copper salts, mercury salts, etc. (Kossel, 1929). When heated to 60 °C with the Mirsky histone reagent (0.34 M mercuric sulfate in 1.88 M sulfuric acid) (Daly et al., 1951), protamine and histone are not precipitated whereas many other proteins precipitate. If the mixture is cooled to 0°C, the mercury salt of protamine is precipitated but histone remains in solution. This phenomenon can be utilized to distinguish protamine from histone. 

Lead is reported to be almost imique in not forming compounds of this tA pe, basic lead nitrate and chloride being the principal products formed when aqueous hexamethylenetetramine solutions are reacted with lead nitrate and lead chloride, respectively - . Complexes are reported ivith salts of lithium, sodium, potassium, copper,. silver, gold, magnesium, calcium, strontium, barium, zinc, cadmium, mercury, aluminum, titanium, lanthanum, cerium, neodymium, yttrium, erbium, thorium, tin, antimcnj, bismuth, chromium, molybdenum, tungsten, uranium, manganese, iron, cobalt, nickel, platinum, and palladium -... 

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