10603-61-9

Basic information

• Product Name: Phenol, 3-(hydroxyamino)-
• CAS NO: 10603-61-9
• Molecular Formula: C6H7NO2
• Molecular Weight: 125.127
• Mol File: 10603-61-9.mol
• Article Data: 6

Chemical Properties

• CAS DataBase Reference: Phenol, 3-(hydroxyamino)-(CAS DataBase Reference)
• NIST Chemistry Reference: Phenol, 3-(hydroxyamino)-(10603-61-9)
• EPA Substance Registry System: Phenol, 3-(hydroxyamino)-(10603-61-9)

Safety Data

• Hazardous Substances Data: 10603-61-9(Hazardous Substances Data)

Upstream product

• 591-27-5 m-Hydroxyaniline 
• 554-84-7 meta-nitrophenol 

Downstream Products

• 97369-45-4 (6-Hydroxy-2-indolyl)-3-phenylacrylnitril 
• 97369-46-5 (4-Hydroxy-2-indolyl)-3-phenylacrylnitril 
• 97369-65-8 N-Benzyliden-3-hydroxyphenylamin-N-oxid 
• 591-27-5 m-Hydroxyaniline 
• 97369-66-9 3-<<(3-Hydroxyphenyl)imino>methyl>-1-methylpyridinium-iodid-N-oxid 
• 20031-38-3 3-nitrosophenol 

Relevant articles and documents

Mechanism and reactivity in perborate oxidation of anilines in acetic acid

Perborate but not percarbonate in acetic acid generates peracetic acid on standing and the peracetic acid oxidation of anilines is fast. The oxidation with a fresh solution of perborate in acetic acid is smooth and second order but the specific oxidation rate increases with increasing [perborate]0 or [boric acid]. Perborate on dissolution affords hydrogen peroxide and a borate; the latter assists the former in the oxidation. The oxidation rates of anilines under identical conditions do not conform to any of the linear free energy relationships but the reaction rates of molecular anilines do. Perborate oxidation proceeds via two reaction paths but the overall oxidation rates of molecular anilines conform to structure reactivity relationships; the transition states do not differ significantly. Analysis of the oxidation rates of perborate and percarbonate reveals that while perborate oxidation is faster than percarbonate it is at least as selective as the latter.

ELECTROCHEMICAL REDUCTION OF m-NITROPHENOL IN BUFFERED AQUEOUS SOLUTIONS

A study on the electrochemical reduction of m-nitrophenol on a mercury electrode in buffered aqueous solutions, has been carried out, focusing on the zone of potentials corresponding to the rising portion of the wave (i/iL0.05), whose corresponding kinetic parameters allow us to suggest a reduction mechanism for each of the pH-ranges of 0-1, 1-8.4, 8.4-10.6, and 10.6-13.5.

Kinetics and Mechanism of Polarographic Reduction of Aromatic Nitro Compounds in Aqueous Alcoholic Medium

Polarographic reduction of nitrobenzene, ortho-, meta- and para- chloronitrobenzenes, nitrotoluenes, nitrophenols and nitrobenzaldehydes has been studied in 25percent (v/v) aqueous ethanolic solutions, using Britton-Robinson (BR) buffer of varying pH values.KCl (0.1 M) has been used as the supporting electrolyte and Triton X-100 (0.001percent) as the maxima suppressor.The potential-dependent rate constant, kf,h has been calculated by Koutecky's method at different pH values and the values of kinetic parameters (αna and kf,h) have been calculated from logkf,h versus Ed.e. plots which are linear thereby suggesting that only a single rate-determining step is involved in the electrode process of each depolarizer.Based on the values of kinetic parameter, αna and the variation of E1/2 with pH, the stoichiometry of the rate-determining step has been established.This has led to the postulation of a tentative mechanism for the polarographic reduction of each depolarizer.Besides, the effect of the nature and position of various substituents, viz.Cl, CH3, OH and CHO on the kinetics of the polarographic reduction of NO2 group has been investigated.