Ferric nitrate, acidity

Chemical Designations - Synonyms Ferric nitrate monahydrate, Nitric acid, iron (+3) salt Chemical Formula Fe(N03)3 9H20. 

The immediate outcome of the Hantzsch synthesis is the dihydropyridine which requires a subsequent oxidation step to generate the pyridine core. Classically, this has been accomplished with nitric acid. Alternative reagents include oxygen, sodium nitrite, ferric nitrate/cupric nitrate, bromine/sodium acetate, chromium trioxide, sulfur, potassium permanganate, chloranil, DDQ, Pd/C and DBU. More recently, ceric ammonium nitrate (CAN) has been found to be an efficient reagent to carry out this transformation. When 100 was treated with 2 equivalents of CAN in aqueous acetone, the reaction to 101 was complete in 10 minutes at room temperature and in excellent yield. 

Besides Fe-, other reducing agents that may be used in conjunction with H2O2 are aliphatic amines, Na2S203 thiourea, ascorbic acid, glyoxal, sulfuric acid, NaHSOs, sodium nitrite, ferric nitrate, peroxidase, AgNOs, tartaric acid, hydroxylamine, ethylene sulfate, sodium phosphite, formic acid, ferrous ammonium sulphate, acetic acid, ferrous sulphate, and HNO2, etc,... 

Fermentation, 22, 53 Ferric nitrate, 23, 20 Fieser s solution, 21, 110 Filter fabric, Pyrex glass, 22, 33, 65 Vinyon, 22, 33, 67 Filter paper, hardened, 22, 45 Fischer indole synthesis, 22, 98 Flash distillation, 21, 85 Flask, modified Claisen, 22, 11 Fluorescence of 9-aminoacridine hydrochloride, 22, 7 Formaldehyde, 20, 60 Formalin, 22, 66 Formic acid, 20, 66, 102 23, 43 Formic acid, chloro-, benzyl ester, 23, 13... 

Catalyst, alumina, 34, 79 35, 73 ammonium acetate, 31, 25, 27 copper chromite, 31, 32 36, 12 cuprous oxide-silver oxide, 36, 36, 37 ferric nitrate, hydrated, 31, 53 piperidine, 31, 35 piperidine acetate, 31, 57 Raney nickel, 36, 21 sulfuric acid, 34, 26 Catechol, 33, 74 Cetylmalonic acid, 34, 16 Cetylmalonic ester, 34,13 Chlorination, by sulfuryl chloride, 33, 45 ... 

Determination in Biological Fluids and Tissues All the advances in pharmacokinetics and drug metabolism described in Sections 7 and 8 would not have been possible without the availability of the proper analytical methods. The following is a tabulation of publications in this field, most of which have already been discussed in Section 5. It should be mentioned that a few publications talk about aspirin blood levels, but really mean salicylate levels. The following tabulation covers only those papers where aspirin was differentiated from other salicylates by chromatography or other means. It seems that the "workhorse" for serum salicylate levels is still the colorimetric (ferric-nitrate) method of Brodie, Udenfriend and Coburn153 published in 1944, or modifications thereof. Simplified versions (cf. 206) may lead to erroneous results under certain conditions.207 The method is also applicable for urinary metabolites after proper hydrolysis (cf. 208). For other methods restricted to salicylic acid, see Section 5.61. 

Ferric citrate, molecular formula, 6 638t Ferric ethoxide, 14 533 Ferric ethylenediaminetetraacetic acid (ferric EDTA), 19 261 Ferric ferrocyanide, 8 186 22 810 pigment used in makeups, 7 836t Ferrichromes, 14 557 Ferric ion, acrylamide stabilizer, 1 289 Ferric nitrate bright pickle, 15 375 Ferric oxide... 

Salicylate has an absorption maximum at 290 nm (A). Complexing with ferric nitrate in an acid results in a shift of the absorption maximum into the visible region at 510 nm (B) and provides the basis for a method of quantitation. 

Buffer solution - dissolve 6.0 g ferric nitrate, Fe(N03)3.9FH20, and 0.15 g silver nitrate, AgNOj, in water and make up to 100 ml add this to a solution of 5.0 g potassium acetate in 500 ml glacial acetic acid in a 2-1 beaker and stir to mix. Add 400 ml 2-methylpropan-2-ol (tertiary butyl alcohol, (CH3)3C0H this solidifies s25.5°C, therefore it may need warming to melt before use), and stir to mix. Store in a brown glass bottle. 

Hot dilute nitric acid reacts with iron, forming ferric nitrate, Fe(N03)3. Also, nitrogen oxides evolve in the reaction, probably from decomposition of... 

Aqueous acid has been utilized to cleave the enamine-like C—N bond of the 9-alkenylcarbazoles 94 and 95 ° and the products 82 of alkylation of the anions of 9-allyIcarbazoles hydrated ferric nitrate was used to remove the vinyl group from 3-halo-9-vinylcarbazoles, Strong base... 

Ferric Nitrate (Iron Nitrate), Fe(N0s)3.9H30 mw 404.02, It viol monocl delq crysts, mp 47°, dec at 100° v sol in w ale. Can be prepd by the action of coned nitric acid on scrap iron or on iron oxide, followed by crystn. It is a strong oxidizing agent and is considered to be dangerous as a fire hazard. Used in analytical chemistry... 

Synonym Neatsfoot Oil Necatorina Nechexane Neutral Ahhonium Pluoride Neutral Anhydrous Calcium Hypochlorite Neutral Lead Acetate Neutral Nicotine Sulfate Neutral Potassium Chromate Neutral Sodium Chromatetanhydrous Neutral Verdigris Nickel Acetate Nickel Acetate Tetrahyorate Nickel Ammonium Sulfate Nickel Ammonium Sulfate Hexahydrate Nickel Bromide Nickel Bromide Trihydrate Nickel Carbonyl Nickel Chloride Nickel Chloride Nickel Cyanide Nickel Iiu Fluoborate Nickel Fluoroborate Solution Nickel Fluoroborate Nickel Formate Nickel Formate Dihyorate Nickel Nitrate Nickel Nitrate Hexahydrate Nickel Sulfate Nickel Tetracarbokyl Nickelous Acetate Nickelous Sulfate Nicotine Nicotine Sulfate Nifos Nitralin Nitram O-Nitraniline P-Nitraniline Nitric Acid Nitric Acid, Aluminum Salt Nitric Acid, Iron (111) Salt Compound Name Oil Neatsfoot Carbon Tetrachloride Neohexane Ammonium Fluoride Calcium Hypochlorite Lead Acetate Nicotine Sulfate Potassium Chromate Sodium Chromate Copper Acetate Nickel Acetate Nickel Acetate Nickel Ammonium Sulfate Nickel Ammonium Sulfate Nickel Bromide Nickel Bromide Nickel Carbonyl Nickel Chloride Nickel Chloride Nickel Cyanide Nickel Fluoroborate Nickel Fluoroborate Nickel Fluoroborate Nickel Formate Nickel Formate Nickel Nitrate Nickel Nitrate Nickel Sulfate Nickel Carbonyl Nickel Acetate Nickel Sulfate Nicotine Nicotine Sulfate Tetraethyl Pyrophosphate Nitralin Ammonium Nitrate 2-Nitroaniline 4-Nitroaniline Nitric Acid Aluminum Nitrate Ferric Nitrate... 

Ferric Nitrate — Fire Hazards Flash Point (deg. F) Not flammable Flammable Limits in Air (%>) Not flammable Fire Extinguishing Agents Not pertinent Fire Extinguishing Agents Not To Be Used Not pertinent Special Hazards of Combustion Products Toxic oxides of nitrogen and nitric acid vapor may form in fires Behavior in Fire In contact with combustible materials, will increase the intensity of a fire Ignition Temperature (deg. F) Not pertinent Electrical Hazard Not pertinent ... 

A. Connell (1802) 140 obtained a white precipitate—ferrous iodate—by boiling a soln. of iron in iodic acid, and C. F. Rammelsberg found that the addition of potassium iodate to ferrous sulphate gives a yellowish-white precipitate which is decomposed when heated. It is sparingly soluble in nitric acid, and it dissolves in an excess of ferrous sulphate, and the soln., when heated, precipitates basic ferric iodate. A. Ditte mixed boiling soln. of a ferric salt and an alkali iodate and obtained a brown precipitate—ferric iodate—insoluble in hot nitric acid diluted with its own volume of water. Crystals can be obtained by mixing warm dil. soln. of ferric nitrate, acidified with nitric acid, and sodium iodate. The precipitate... 

Supersaturation.—One of the most frequent difficulties in crystallization is due to super saturation. This condition arises when the normal saturation concentration of a salt solution is exceeded without the appearance of any crystals, and as the solution cools further it becomes steadily more supersaturated. When crystallization finally starts, it proceeds with great rapidity, forming a mass of poorly defined crystals unsuited to drying. The tendency toward supersaturation is most marked in the case of very soluble substances which form viscous or syrupy solutions. Lead acetate, sodium thiosulfate, ferric nitrate, and sulfuric acid are good examples. 

Like ferric nitrate, antimony sulfate is decomposed by water, various basic salts being formed, the simplest of which has the formula (SbOLSCL. The normal salt is stable only in rather concentrated sulfuric acid. Since this latter solvent has almost no vapor pressure at ordinary temperatures, the moist salt cannot be dried by evaporation of the solvent. It cannot be dried on absorbent paper, since the oily liquid rapidly carbonizes it. In such a case, it is best to take advantage of the drying qualities of unglazed earthenware (porous plate), such as the biscuit which forms the body of dishes. Owing to the fine pores which this material contains, liquids are sucked up by it by capillary attraction, and it is not acted upon by most reagents. 

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