108-07-6

Usage

Uses

Used in Research and Development:
Methyl mercuric acetate may be used in controlled research and development settings for specific scientific purposes, such as studying the effects of heavy metals on biological systems or developing methods for detecting and analyzing mercury compounds. In these cases, it is essential to follow strict safety guidelines and use appropriate protective equipment to minimize the risk of exposure.
Used in Analytical Chemistry:
In some instances, methyl mercuric acetate may be used as a reagent or standard in analytical chemistry for the determination of trace amounts of mercury or other related compounds. However, due to its toxicity, it should only be used in well-controlled laboratory environments with proper safety measures in place.
It is important to emphasize that the use of methyl mercuric acetate should be limited to these specific applications and conducted under strict safety conditions. The potential health risks associated with exposure to this substance far outweigh any potential benefits, and its use should be avoided whenever possible in favor of safer alternatives.

InChI:InChI=1/C2H4O2.CH3.Hg/c1-2(3)4;;/h1H3,(H,3,4);1H3;/rC2H4O2.CH3Hg/c1-2(3)4;1-2/h1H3,(H,3,4);1H3

Upstream product

• 1600-27-7 mercury(II) diacetate 
• 593-74-8 dimethylmercury 
• 143-36-2 methylmercury(II) iodide 
• 64-19-7 acetic acid 
• 110-22-5 diacetyl peroxide 
• 13213-27-9 cyclohexyl-1,1-diacetylperoxide 
• 594-27-4 tetramethylstannane 
• 631-60-7 mercury(I) acetate 
• 546-67-8 lead(IV) tetraacetate 
• 94-36-0 dibenzoyl peroxide 
• 22967-92-6 methylmercury(II) 
• 563-63-3 silver(I) acetate 

Downstream Products

• 108-24-7 acetic anhydride 
• 25310-48-9 Methylquecksilber-methylmercaptid 
• 593-74-8 dimethylmercury 
• 1907-13-7 acetoxytriethylstannane 
• 91258-91-2 β-methylmercury-4-fluorophenylacetylene 
• 84839-18-9 (CH₃O)3Si(CH₂)SHgCH₃ 

Relevant academic research and scientific papers

1H NMR Rate Constants and Mercury-199 FT NMR Equilibrium Constants Involved in Disulfide Cleavage by Methylmercury

A 1H NMR kinetic investigation of the cleavage of dimethyl disulfide with methylmercury acetate and triethyl phosphite is described.The metal-assisted -SS- bond rupture is first order in both CH3HgII and CH3SSCH3.Mercury-199 FT NMR has been employed to measure the equilibrium constants for complexation of CH3HgOAc with CH3SSCH3 and P(OEt)3.A concomitant electrophilic and nucleophilic mechanism for -SS- bond cleavage is suggested that involves attack by P(OEt)3 on the -SS- ?* orbital of the CH3HgII complex of CH3SSCH3.

A Raman spectroscopic study of the complexation of the methylmercury(II) cation by amino acids

A systematic Raman spectroscopic investigation of the complexation of CH3Hg(1+) by the standard amino acids is reported.It is shown that the vibrational bands due to the ligand-Hg and Hg-CH3 stretching modes and to the symmetric -CH3 bending mode of the -HgCH3 unit are well suited to characterize the extent of complexation and the sites of attachment of the cation.Coordination, which occurs mostly on sulfur and nitrogen atoms by substitution of a proton on the thiol group of cysteine or on amino groups in general, is best identified by the frequency of the ligand-Hg stretching vibration in the 250-550 cm-1 region of the spectrum.

A 199Hg FT-NMR and X-ray structural study of the interaction of MeHgII with pyridines. The effect of solvent and steric interactions

A 199Hg FT-NMR study on the extent of complexation of methylmercury with a series of pyridines is described. The formation constants decrease as the steric hindrance around the nitrogen increases in both methylene chloride and nitromethane solvents. However, in methanol solvent one sees a reversal of trends in that the Kf increases on going from pyridine to 2-methylpyridine and levels off with the more hindered 2,6-dimethylpyridine. The increase in complexation is attributed to a ground-state solvation effect on the pyridines. The decrease in hydrogen bonding of the more hindered nitrogenous bases increases their Lewis basicity. An X-ray structural study on the complex of 2-methylpyridine with methylmercury(II) trifluoroacetate shows that the C-Hg-N is nearly linear with trifluoroacetate anion being weakly bound to two mercury atoms forming a losely associated dimeric complex with Hg-O bridging distances of 2.668 (9) and 2.805 (8) ?.

Electron-Transfer Activation in Electrophilic Mechanisms. Cleavage of Alkylmetals by Mercury(II) Complexes

The disappearance of the transient charge-transfer (CT) absorption bands coincides with the electrophilic (SE2) cleavage of homologous series of alkyltin compounds by various mercury(II) halides, cyanide, and carboxylates.The second-order kinetics for HgCl2 cleavage afford rate constants which vary in a rather unaccountable way with the structure of the alkyltin compound and with the polarity of the solvent.Furthermore, the relative reactivities of these alkyltin compounds in the analogous electrophilic cleavage by I2 or Br2 show poor correlations with HgCl2 cleavages, in different solvents.However, the description of the activation process as an electron transfer in the precursor complex, e.g., -> +HgCl2->, stems from the CT transition energy and leads to a linear free energy relationship in which the activation free energy is equal to the driving force for the formation of the ion pair.The latter is readily dissected by eq 18 into separate changes in electronic, steric and solvation energies.With this mechanistic formulation, the reactivities of various alkyltin compounds follow a remarkably simple linear correlation with the ionization potentials and the solvent effects, in the comparison with I2 and Br2 cleavages.Moreover, the reactivities of the various mercury(II) derivatives relate directly to differences in their electron affinities.