20758-58-1

Upstream product

• 5878-19-3 Methoxyacetone 
• 184582-82-9 C₃H₆NO₄^(1-) 
• 625-45-6 2-methoxyacetic acid 
• 188819-30-9 C₂H₄NO₃^(1-) 
• 196078-73-6 2,4,6-trimethylphenyl methoxyacetate 

Downstream Products

• 53103-76-7 methoxy-acetic acid methoxymethyl ester 
• 27610-20-4 substituted benzenethiol 
• 126083-72-5 C₁₃H₆N₅O₁₀^(1-) 
• 126083-71-4 (2,2',4,4',6,6'-hexanitro-diphenyl)-methyl anion 
• 188819-30-9 C₂H₄NO₃^(1-) 
• 625-45-6 2-methoxyacetic acid 
• 184582-82-9 C₃H₆NO₄^(1-) 

Relevant academic research and scientific papers

Degenerate transesteriflcation of dimeric lithium 2,4,6-trimethylphenolate and a further observation on the reaction of tetramers

The rates of exchange of the 2,4,6-trimethylphenolate ion between dimeric lithium 2,4,6-trimethylphenolate-d9 and a series of 2,4,6-trimethylphenyl esters [2,4,6-(CH3)3C6H2COOCH2R; R = CHs

Kinetics of reversible carbon deprotonation of 2-nitroethanol and 2-nitro-1,3-propanediol by hydroxide ion, water, amines, and carboxylate ions. A normal br?nsted α despite an imbalanced transition state

Rates of reversible carbon deprotonation of 2-nitroethanol (2) and 2-nitro-1,3-propanediol (3) by hydroxide ion, water, amines, and carboxylate ions and pKa values for the ionization at carbon (pKaCH) and oxygen (pKaOH) and ionization of the aci-forms (pKaNOH) were determined in aqueous solution at 25 °C. The pKaCH values for 2 and 3 are 8.60 and 7.68, respectively, as compared to 10.22 for CH3NO2. The acidifying effect of the CH2OH groups is attributed to a combination of inductive electron withdrawal and hyperconjugative stabilization of the respective nitronate ions, possibly coupled with intramolecular hydrogen bonding stabilization of this ion. The higher acidity of 2-nitroethanol compared to nitromethane is reflected in higher rates of proton transfer from 2-nitroethanol, implying a "normal" Br?nsted α between 0 and 1. This contrasts with the negative α value based on the reaction of OH- with nitromethane, nitroethane, and 2-nitropropane (Kresge, A. J. Can. J. Chem. 1974, 52, 1897). Reasons why a normal α value is observed in the current system are discussed.

Halogenation of Acetone. A Method for Determining pKas of Ketones in Aqueous Solution, with an Examination of the Thermodynamics and Kinetics of Alkaline Halogenation and a Discussion of the Best Value for the Rate Constant for a "Diffusion-Controlled Reaction". Energetic ...

The pKa of a simple ketone can be determined by analysis of the kinetics of halogenation in alkaline solution (J.Am.Chem.Soc. 1982, 104, 895).Details of the determination of the pKa of acetone are reported.The stoichiometry of chlorination of acetone is 2.15 hypohalites per acetone; bromination consumes 2.83 hypobromites.The major product from chlorination is lactate and not acetate; lactate is a minor product from bromination of acetone.The kinetic significance of the possible side reactions is discussed.The determination of the pKa requires knowledge of the rate constant for a diffusion-controlled reactionof nonspherically symmetrical molecules in water; the state of our knowledge of this rate constant is reviewed critically.It is shown that for reactions involving diffusion together of reactants which then undergo direct heavy-atom bond making it is very unusual for the diffusion limit to be reached, although the observed rate constant may become insensitive to the thermodynamic rectivity of the reactants.