16090-33-8

Basic information

• Product Name: 2-NITROHYDROQUINONE
• Synonyms: 2-NITROHYDROQUINONE;TIMTEC-BB SBB008501;2-NITROHYDROQUINONE ---ORANGE RED CRYSTALS---;2-Nitro-4-hydroxyphenol;2-Nitrobenzene-1,4-diol;2-Nitroquinol;4-Hydroxy-2-nitrophenol;Nitrohydroquinone
• CAS NO: 16090-33-8
• Molecular Formula: C₆H₅NO₄
• Molecular Weight: 155.11
• Mol File: 16090-33-8.mol
• Article Data: 18

Chemical Properties

• Melting Point: 133-134℃
• Boiling Point: 278.88°C (rough estimate)
• Flash Point: 143.2ºC
• Appearance: /
• Density: 1.5553 (rough estimate)
• Vapor Pressure: 0.000423mmHg at 25°C
• Refractive Index: 1.5423 (estimate)
• Storage Temp.: under inert gas (nitrogen or Argon) at 2-8°C
• Solubility: Chloroform (Slightly, Heated), Dichloromethane (Slightly)
• PKA: pK1:7.63;pK2:10.06 (25°C)
• Water Solubility: 10.68g/L(30.20 oC)
• CAS DataBase Reference: 2-NITROHYDROQUINONE(CAS DataBase Reference)
• NIST Chemistry Reference: 2-NITROHYDROQUINONE(16090-33-8)
• EPA Substance Registry System: 2-NITROHYDROQUINONE(16090-33-8)

Safety Data

• Hazardous Substances Data: 16090-33-8(Hazardous Substances Data)

Usage

General Description

2-Nitrohydroquinone is a chemical compound with the molecular formula C6H5NO3. It is a colorless to light yellow solid that is used in the production of dyes and pharmaceuticals. 2-Nitrohydroquinone is synthesized through the nitration of hydroquinone, and it is commonly used as a reagent in organic synthesis and as an intermediate in the manufacture of antioxidants and photographic developers. It is also used in the production of hair dyes and in the treatment of certain skin conditions. 2-Nitrohydroquinone is classified as a hazardous substance and must be handled and stored with care to prevent exposure and environmental contamination.

InChI:InChI=1/C6H5NO4/c8-4-1-2-6(9)5(3-4)7(10)11/h1-3,8-9H

Upstream product

• 554-84-7 meta-nitrophenol 
• 2444-19-1 4-hydroxyphenyl benzoate 
• 13985-43-8 4-hydroxy-3-nitrophenyl benzoate 
• 89-39-4 1,4-dimethoxy-2-nitrobenzene 
• 88-75-5 2-hydroxynitrobenzene 
• 123-31-9 hydroquinone 
• 98-95-3 nitrobenzene 

Downstream Products

• 1568-69-0 Allyl-(3-nitro-4-hydroxy-phenyl)-aether 
• 89-39-4 1,4-dimethoxy-2-nitrobenzene 
• 103261-93-4 (3-acetoxy-4-nitro-phenyl) acetate 
• 51792-85-9 (((2-nitro-1,4-phenylene)bis(oxy))bis(methylene))dibenzene 
• 1417795-71-1 C₁₃H₉NO₄ 

Relevant articles and documents

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Sodium perborate/NaNO2/KHSO4-triggered synthesis and kinetics of nitration of aromatic compounds

Sodium perborate (SPB) was used as efficient green catalyst for NaNO2/KHSO4-mediated nitration of aromatic compounds in aqueous acetonitrile medium. Synthesis of nitroaromatic compounds was achieved under both conventional and solvent-free microwave conditions. Reaction times were comparatively shorter in the microwave-assisted than conventional reaction. The reaction kinetics for nitration of phenols in aqueous bisulfate and acetonitrile medium indicated first-order dependence on [Phenol], [NaNO2], and [SPB]. Reaction rates accelerated with introduction of electron-donating groups but retarded with electron-withdrawing groups. Kinetic results did not fit well quantitatively with Hammett’s equation. Observed deviations from linearity were addressed in terms of exalted Hammett’s constants (σˉ or σeff), para resonance interaction energy (ΔΔGp) parameter, and Yukawa–Tsuno parameter (r). This term provides a measure of the extent of resonance stabilization for a reactive structure that builds up charge (positive) in its transition state. The observed negative entropy of activation (?ΔS#) suggests greater solvation and/or cyclic transition state before yielding products.

Prussian Blue/NaNO2 as an Efficient Reagent for the Nitration of Phenols in Aqueous Bisulfate and Acetonitrile Medium: Synthetic and Kinetic Study

The reaction kinetics of Prussian blue (PB)/NaNO2 initiated for the nitration of phenols by in aqueous bisulfate and acetonitrile medium indicated first-order dependence on [phenol], [NaNO2], and [PB]. An increase in [KHSO4] accelerated the rate of nitration under otherwise similar conditions. The rate of nitration was faster in the solvent of higher dielectric constant (D). Observed results were in accordance with Amis and Kirkwood plots [log k′ vs. (1/D) and [(D ? 1)/(2D + 1)]. These findings together with the linearity of plots, log k′ versus (vol% of acetonitrile (ACN)) and mole fraction of (nx) ACN, probably indicate the importance of both eloctrostatic and nonelctrostatic forces, solvent–solute interactions during nitration of phenols. Reaction rates accelerated with the introduction of electron-donating groups and retarded with electron-withdrawing groups, which are interpreted by Hammett's theory of linear free energy relationship. Hammett's reaction constant (ρ) is a fairly large negative (ρ 0) value, indicating attack of an electrophile on the aromatic ring. Furthermore, an increase in temperature decreased the reaction constant (ρ) values. This trend was useful in obtaining isokinetic temperature (β) from Exner's plot of ρ versus 1/T. Observed β value (337.8 K) is above the experimental temperature range (303–323 K), indicating that the enthalpy factors are probably more important in controlling the reaction.