7782-61-8 Usage
Description
Iron(III) Nitrate Nonahydrate is a highly water soluble crystalline Iron source for uses compatible with nitrates and lower (acidic) pH. All metallic nitrates are inorganic salts of a given metal cation and the nitrate anion. The nitrate anion is a univalent (-1 charge) polyatomic ion composed of a single nitrogen atom ionically bound to three oxygen atoms (Formula: NO3) for a total formula weight of 62.05.
Uses
Different sources of media describe the Uses of 7782-61-8 differently. You can refer to the following data:
1. Ferric nitrate nonahydrate can be used as catalyst, mordant, metal surface treatment agent, oxidant, analytical reagent, radioactive substance adsorbent.
2. Ferric nitrate nonahydrate is used as a mordant for dyeing black and buff. Other applications are in tanning; weighting silks; and in preparation of analytical standards.
3. Ferric nitrate nonahydrate is used in the determination of phosphate.
4. It is used as catalyst for the synthesis of sodium amide from sodium and ammonia, and for etching of silver and silver alloys. Ferric nitrate is used in the synthesis of organically templated iron phosphates, and acts as an efficient catalyst in enamination of beta dicarbonyl compounds to beta enaminones. Ferric nitrate impregnated clays are useful as oxidizing agents. Clayfen, produced from ferric nitrate and montmorillonite, is used for the oxidation of thiols to disulfide, and alcohols to aldehydes. Ferric nitrate is useful for regio- and stereo-selective nitration of various aromatic, aliphatic, and heteroaromatic olefins. This reaction provides nitroolefins with excellent E-selectivity. With Keggin-type heteropoly acids, it selectively oxidizes various hydroxy groups.
analysis method
Weigh 1~1.5g sample (accurate to 0.0001g) into a 250ml dry iodine measuring flask, and record the weight m. Add 20ml of water, 3g of potassium iodide, and 10ml of sulfuric acid solution (10%), and shake it up to dissolve completely, place in a dark place for 10-15 minutes, add about 80ml of water, titrate with sodium thiosulfate standard titration solution, and add when near the end 3ml starch indicator solution, continue to titrate until the blue color of the solution fades as the end point.
V--The value of the volume of sodium thiosulfate standard titration solution, in milliliter (mL);
c--The exact value of the concentration of sodium thiosulfate standard titration solution, the unit is moles per liter (mol/L);
0.404- -The mass of iron nitrate [(Fe (NO3) 3●9H2O)] equivalent to 1.00mL with sodium thiosulfate standard titration solution [C (Na2S2O3)=0.1000mol/L] in grams;
m---Sample mass, g.
Preparation
In the iron filing method, nitric acid with a relative density of 1.38 is added to an acid-resistant reactor filled with water, heated to 40-50°C, and fine iron filings are slowly added to react for 3 hours. The solution is heated to drive out the nitrogen oxide gas. Filter, evaporate and concentrate the filtrate to form a crystal film, send it to a cooling crystallizer to cool to below 0°C to precipitate crystals. After suction filtration, the crystals are washed with 20% nitric acid. The finished Ferric nitrate nonahydrate is produced. The reaction formula is as follows. Fe+4HNO3→Fe(NO3)3+NO+2H2OFe+6HNO3→Fe(NO3)3+3NO2+3H2O
The mother liquor can be recycled. The nitrogen oxide gas released during the reaction is commonly absorbed by caustic soda solution in industry. Because of its fast absorption rate, the obtained neutralization liquid is used to produce sodium nitrate.
General Description
This product has been enhanced for catalytic efficiency.
Purification Methods
It crystallises from aqueous solutions of moderately strong HNO3 as the pale violet nonahydrate m 40o and is soluble in EtOH and Me2CO. With more concentrated aqueous solutions (containing some HNO3), the hexahydrate crystallises out m 60.5o . The anhydrous salt is slightly deliquescent and decomposes at 47o. [Lambert & Thomson J Chem Soc 97 2426 1920, Gmelin’s, Iron (8th edn) 59 Part B pp 161-172 1932.]
Check Digit Verification of cas no
The CAS Registry Mumber 7782-61-8 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 7,7,8 and 2 respectively; the second part has 2 digits, 6 and 1 respectively.
Calculate Digit Verification of CAS Registry Number 7782-61:
(6*7)+(5*7)+(4*8)+(3*2)+(2*6)+(1*1)=128
128 % 10 = 8
So 7782-61-8 is a valid CAS Registry Number.
InChI:InChI=1/Fe.3NO3.9H2O/c;3*2-1(3)4;;;;;;;;;/h;;;;9*1H2/q+3;3*-1;;;;;;;;;
7782-61-8Relevant articles and documents
Environmentally Benign Solution-Based Procedure for the Fabrication of Metal Oxide Coatings on Metallic Pigments
Bies, Thorsten,Hoffmann, Rudolf C.,Huber, Adalbert,Schneider, J?rg J.,St?ter, Matthias
, p. 1251 - 1263 (2020)
Aluminum pigments were coated with Fe2O3 and CuO by solution-based thermal decomposition of the urea nitrate compounds hexakisureairon(III)nitrate and tetrakisureacopper(II)nitrate. The deposition process was optimized to obtain homo
The kinetics of hydrochemical oxidation of iron(II) persulfide (pyrite) by nitric acid
Sobolev,Lutsik,Potashnikov
, p. 757 - 759 (2007/10/03)
The kinetics of pyrite oxidation by nitric acid was studied by the rotating disk method. The conditions of kinetically and diffusion-controlled processes were determined. At nitric acid concentrations below 9 mol/dm3, the reaction proceeded in a mixed mode close to kinetically controlled, and the products of acid reduction had an autocatalytic action on the rate of pyrite oxidation. At HNO3 concentrations exceeding 11 mol/dm3, the reaction proceeded in a mixed mode close to diffusion-controlled, and the rate of the reaction sharply decreased. The reason why pyrite reacted with concentrated nitric acid at a low rate was a decrease in the solubility of reaction products.
Investigation of montmorillonite-based clays in the preparation of supported ferric nitrate
Bekassy, Sandor,Cseri, Tivadar,Bodas, Zoltan,Figueras, Francois
, p. 357 - 364 (2008/10/08)
A series of montmorillonite-based clays (KSF, KSF/0, K0, KP10, K10, KS from Sued-Chemie) were obtained by treating a Bavarian bentonite with different acids and a Hungarian bentonite (Mad), and were used for the preparation of supported hydrated iron(III) nitrates. The clay supports were characterized by different methods (chemical analysis, nitrogen adsorption, X-ray powder diffraction, thermal analysis and solid-state NMR) and the acidity of these solids was determined by infrared spectroscopy using pyridine as a molecular probe. The supported iron nitrate reagents were investigated by thermal and X-ray powder diffraction methods. The iron nitrate is present on the support as an amorphous hydrate. The decomposition of the nitrate is shifted towards lower temperature when it is supported and starts at 35-40 C. The supported iron nitrate reagents show high activities and selectivities in the oxidation of benzyl alcohol to benzaldehyde. The high specific surface area and the Bronsted acidity of the support are determining factors for the chemical activity of the supported system. The supported reagents prepared according this procedure can be stocked for as long as six months without any loss of chemical properties. CNRS-Gauthier-Villars.
