7782-61-8

Basic information

• Product Name: Ferric nitrate nonahydrate
• Synonyms: IRON(+3)NITRATE ENNEAHYDRATE;IRON (III) NITRATE;IRON(III) NITRATE-9-HYDRATE;IRON(III) NITRATE ENNEAHYDRATE;IRON (III) NITRATE, HYDROUS;IRON(III) NITRATE NONAHYDRATE;IRON(III) NITRATE, NONOHYDRATE;FERRIC NITRATE 9H2O
• CAS NO: 7782-61-8
• Molecular Formula: Fe*3NO₃
• Molecular Weight: 404
• EINECS: 233-899-5
• Product Categories: metal nitrate salts
• Mol File: 7782-61-8.mol

Chemical Properties

• Melting Point: 47 °C(lit.)
• Boiling Point: 125°C
• Flash Point: 125°C
• Appearance: White to gray or light purple/Solid
• Density: 1,68 g/cm3
• Storage Temp.: Store at RT.
• Water Solubility: soluble
• Sensitive: Moisture Sensitive
• Stability: Stable. Strong oxidizer - contact with combustible material may lead to fire. Incompatible with combustible material, strong red
• Merck: 14,4027
• CAS DataBase Reference: Ferric nitrate nonahydrate(CAS DataBase Reference)
• NIST Chemistry Reference: Ferric nitrate nonahydrate(7782-61-8)
• EPA Substance Registry System: Ferric nitrate nonahydrate(7782-61-8)

Safety Data

• Hazard Codes: O,Xi,C
• Statements: 8-36/37/38-34
• Safety Statements: 17-26-36-24/25-45-36/37/39-28
• RIDADR: UN 1466 5.1/PG 3
• WGK Germany: 1
• RTECS: NO7175000
• F: 3-9-23
• TSCA: Yes
• HazardClass: 5.1
• PackingGroup: III
• Hazardous Substances Data: 7782-61-8(Hazardous Substances Data)

Usage

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.]

InChI:InChI=1/Fe.3NO3.9H2O/c;3*2-1(3)4;;;;;;;;;/h;;;;9*1H2/q+3;3*-1;;;;;;;;;

Synthetic route

(CH3)3SiCHCH2(SFe(CO)3)2 + nitric acid (7697-37-2) → ferric nitrate (7782-61-8) + ethenyltrimethylsilane (754-05-2)

Conditions	Yield
In nitric acid byproducts: H2SO4, NO, CO; stirring for 0.5 h at 25°C; condensing silane in a trap cooled with solid CO2, treating aq. layer with NaOH, evapn. to dryness, IR;	A n/a B 99%

(CH3)2Si(CH2CHSFe(CO)3)2 + nitric acid (7697-37-2) → 1,1-Dimethylsilacyclopent-3-en (16054-12-9) + ferric nitrate (7782-61-8)

Conditions	Yield
In nitric acid byproducts: H2SO4, NO, CO; stirring for 0.5 h at 25°C; condensing silane in a trap cooled with solid CO2, treating aq. layer with NaOH, evapn. to dryness, IR;	A 96% B n/a

iron(III) oxide + nitric acid (7697-37-2) → ferric nitrate (7782-61-8)

Conditions	Yield
In water dissolving of Fe2O3 in excess of HNO3 for 30 - 45 days; not isolated, measuring of conc. of Fe(3+) by photometrically;

nitric acid (7697-37-2) + iron (7439-89-6) → ferric nitrate (7782-61-8)

Conditions	Yield
In nitric acid Fe is dissolved in dild. HNO3 with evolution of gas, formation of Fe(NO3)3;;
In nitric acid byproducts: basic iron(III)nitrate; Fe is dissolved in HNO3 (d = 1.115), formation of Fe(NO3)3 and basic iron(III)nitrate;;
In nitric acid byproducts: basic iron(III)nitrate; aq. HNO3; Fe is dissolved in HNO3 (d = 1.115), formation of Fe(NO3)3 and basic iron(III)nitrate;;
In nitric acid aq. HNO3; Fe is dissolved in dild. HNO3 with evolution of gas, formation of Fe(NO3)3;;
In ethanol; water for 24h;

nitric acid (7697-37-2) + iron (7439-89-6) → iron(II) nitrate + ferric nitrate (7782-61-8)

Conditions	Yield
In nitric acid storing of Fe for a longer period of time in fuming HNO3;;
In nitric acid storing of Fe for a longer period of time in fuming HNO3;;

nitric acid (7697-37-2) + iron (7439-89-6) → iron(II) nitrate + ammonium nitrate + ferric nitrate (7782-61-8)

Conditions	Yield
In nitric acid Fe is dissolved in HNO3 (d = 1.073), formation of a mixture of Fe(NO3)2 Fe(NO3)3 and NH4NO3;;
In nitric acid aq. HNO3; Fe is dissolved in HNO3 (d = 1.073), formation of a mixture of Fe(NO3)2 Fe(NO3)3 and NH4NO3;;

nitric acid (7697-37-2) + iron (7439-89-6) → ammonia (7664-41-7) + Nitrogen dioxide (10102-44-0) + ferric nitrate (7782-61-8)

Conditions	Yield
In nitric acid Fe is dissolved in HNO3 (34%, d =1.21), at the beginning Fe is dissolved quickly with evolution of gas, then slowly without evolution of gas and formation of Fe(NO3)3 and traces of NO2 and NH3;;
In nitric acid aq. HNO3; Fe is dissolved in HNO3 (34%, d =1.21), at the beginning Fe is dissolved quickly with evolution of gas, then slowly without evolution of gas and formation of Fe(NO3)3 and traces of NO2 and NH3;;

iron(III) sulfate + ammonium hydroxide + nitric acid (7697-37-2) → Ammonium + Sulfate (14808-79-8) + ferric nitrate (7782-61-8)

Conditions	Yield
In water addn. of 10 % soln. of NH4OH to soln. of Fe-salt (pptn.), filtration, washing (hot water) to remove NH4(1+), and SO4(2-), redissolving of Fe(OH)3 in 0.5 M HNO3;

iron pentacarbonyl (13463-40-6) + nitric acid (7697-37-2) → iron(II) nitrate + ferric nitrate (7782-61-8)

Conditions	Yield
In tetrachloromethane byproducts: CO, H2, nitrogen oxides;
In diethyl ether byproducts: CO, H2, nitrogen oxides;

iron (7439-89-6) → ferric nitrate (7782-61-8)

Conditions	Yield
With nitric acid In nitric acid dissoln. of Fe in HNO3 (d > 1.115); formation of Fe(NO3)3 and basic iron nitrates;;
With nitric acid In nitric acid byproducts: HNO2; dissoln. of Fe in a 20-fold excess of HNO3 at 8°C; first formation of Fe(NO3)2, which is oxidized by formed HNO2 to Fe(NO3)3;;
With nitric acid In nitric acid dissoln. of Fe in HNO3 (d = 1.115); formation of Fe(NO3)3;;

iron pentacarbonyl (13463-40-6) → ferric nitrate (7782-61-8)

Conditions	Yield
In nitric acid fast react.;;

nitrosyl tetranitratoferrate(III) → ferric nitrate (7782-61-8)

Conditions	Yield
In neat (no solvent) heating (p(N2O4)=2.0 MPa, 105-135°C); DTA;

potassium perferrate → ferric nitrate (7782-61-8)

Conditions	Yield
With nitric acid byproducts: KNO3, H2O, O2; nascent oxygen formed;
With HNO3 byproducts: KNO3, H2O, O2; nascent oxygen formed;

pyrite + nitric acid (7697-37-2) → ferric nitrate (7782-61-8)

Conditions	Yield
In water Kinetics; byproducts: H2SO4, NO, NO2; heating of aq. soln. of HNO3 with rotating disk from natural pyrite crystals at 303 - 333 K;

iron (7439-89-6) → iron(II) nitrate + ferric nitrate (7782-61-8)

Conditions	Yield
With nitric acid In nitric acid dissoln. of Fe in HNO3 (d > 1.05) at lower temp.; formation of Fe(NO3)2 and Fe(NO3)3;;
With HNO3 In nitric acid aq. HNO3; dissoln. of Fe in HNO3 (d > 1.05) at lower temp.; formation of Fe(NO3)2 and Fe(NO3)3;;

iron(II) nitrate → ferric nitrate (7782-61-8)

Conditions	Yield
With nitric acid In water heating an aq. soln. of Fe(NO3)2 with HNO3; formation of Fe(NO3)3;;
With HNO3 In water heating an aq. soln. of Fe(NO3)2 with HNO3; formation of Fe(NO3)3;;

iron(II) fluoride → iron(III) fluoride (7783-50-8) + ferric nitrate (7782-61-8)

Conditions	Yield
With nitric acid In water discoloration of the aq. soln. of FeF2 with HNO3; formation of FeF3 and Fe(NO3)3;; pptn. as a solid mixt. on evapn.;;
With HNO3 In water discoloration of the aq. soln. of FeF2 with HNO3; formation of FeF3 and Fe(NO3)3;; pptn. as a solid mixt. on evapn.;;

iron(III) nitrate monohydrate → ferric nitrate (7782-61-8)

Conditions	Yield
In solid byproducts: H2O; 160°C to 170°C;

ferric nitrate (7782-61-8) + 3-hydroxy-3,4-dihydrobenzotriazine-4-one (28230-32-2) → tris[3-hydroxy-1,2,3-benzotriazine-4(3H)-one]iron(III) (261168-39-2)

Conditions	Yield
With triethylamine In tetrahydrofuran	100%

zinc(II) nitrate (10196-18-6) + ferric nitrate (7782-61-8) + nickel(II) nitrate → nickel zinc ferrite

Conditions	Yield
With 1,2-ethanediol In water byproducts: C2H2O4(2-); by thermal decompn. of complex combination isolated in heat by oxidn. inaq. soln. of 1,2-ethanediol to C2H2O4(2-) by Ni(II), Zn(II), Fe(III) ni trates; heated at 500-900°C for 3 h; detd. by XRD;	100%

2,6-dimethyl-3,5-heptanedione (18362-64-6) + ferric nitrate (7782-61-8) → tris(2,6-dimethyl-3,5-heptanedionato)iron(III)

Conditions	Yield
With sodium methylate In methanol at 25 - 28℃; for 1.5h;	95.9%

ferric nitrate (7782-61-8) + nickel(II) nitrate → nickel(II) ferrite

Conditions	Yield
With ammonia In water High Pressure; soln. of nitrates, adjustment of pH to 8.66 (ammonia), heating at 192°C for 2 h (microwaves); centrifugation, washing; powder X-ray diffraction;	95%
With ammonia In water High Pressure; soln. of nitrates, adjustment of pH to 8.66 (ammonia), heating at 164°C for 2 h (microwaves); centrifugation, washing; powder X-ray diffraction;	88%
With ammonia In water High Pressure; soln. of nitrates, adjustment of pH to 8.66 (ammonia), heating at 164°C for 4 mins. (microwaves); centrifugation, washing; powder X-ray diffraction;	85%

sodium 2-ethylhexyl carboxylate + ferric nitrate (7782-61-8) → iron(III) 2-ethylhexyl carboxylate

Conditions	Yield
In hexane; water at 40℃;	95%

ferric nitrate (7782-61-8) + cobalt(II) nitrate → cobalt ferrite + iron oxide

Conditions	Yield
With ammonia In water High Pressure; soln. of nitrates, adjustment of pH to 8.71 (ammonia), heating at 164°C for 4 mins. (microwaves); centrifugation, washing; powder X-ray diffraction;	A 94% B n/a

α1-K10[P2W12Mo5O61]*20H2O K10[P2W12Mo5O61]*20H2O, α1 + potassium chloride + ferric nitrate (7782-61-8) → α2-K7[Fe(OH2)P2W13Mo4O61]*15H2O

Conditions	Yield
In water P-compd. was dissolved in the excess of 0.14 M aq. Fe-salt, stirring for10 min, solid KCl was added then soln. was treated with satd. aq. KCl; solid was filtered off, dried in air, elem. anal.;	94%

bismuth(III) nitrate + ammonium hydroxide (1336-21-6) + hexaammonium heptamolybdate tetrahydrate + ferric nitrate (7782-61-8) → Bi3Mo2FeO12

Conditions	Yield
In water at 60 - 550℃; pH=5.0;	94%

manganese(II) nitrate + ferric nitrate (7782-61-8) → manganese ferrite

Conditions	Yield
With ammonia In water High Pressure; soln. of nitrates, adjustment of pH to 8.73 (ammonia), heating at 164°C for 4 mins. (microwaves); centrifugation, washing; powder X-ray diffraction;	92%
With ammonia In water High Pressure; soln. of nitrates, adjustment of pH to 8.95 (ammonia), heating at 164°C for 2 h (microwaves); centrifugation, washing; powder X-ray diffraction;	90%
With ammonia In water High Pressure; soln. of nitrates, adjustment of pH to 8.90 (ammonia), heating at 192°C for 2 h (microwaves); centrifugation, washing; powder X-ray diffraction;	81%

bismuth(III) nitrate + ferric nitrate (7782-61-8) → bismuth ferrite

Conditions	Yield
With nitric acid; tartaric acid In neat (no solvent) nitrates dissolved in HNO3, tartaric acid added, evapd. by heating understirring, heated at 150 - 160 °C for 1 h, calcined at 400 - 600 °C for 2 h; powder XRD, TG;	92%
With citric acid In neat (no solvent) sols prepared from soln. of nitrates and citric acid in ethylene glycol monomethyl ether (Bi excess), spin coated, dried at 80 °C for 30 min, annealed at 200 and 400 °C for 5 min after each coating, annealed at 630 °C for 300-400 s; powder XRD;
In water Bi- and Fe-nitrates in 1.05:1 molar ratio dissolved in double distd. H2Owith few drops of nitric acid under constant heating and stirring for 1 h, sprayed on LaAlO3 substrate maintained at 300+/-5 °C;

Sodium borate + sodium nitrate (7631-99-4) + ammonium molybdate + bismuth subcarbonate + silica gel (112926-00-8, 7631-86-9) + ferric nitrate (7782-61-8) + potassium nitrate + cobalt(II) nitrate + nickel(II) nitrate → B0.2Bi5Co2Fe0.4K0.08Mo12Na0.2Ni3Si24

Conditions	Yield
With oxygen In water at 300℃; for 1h;	91.6%

...Expand

ferric nitrate (7782-61-8) + cobalt(II) nitrate → cobalt ferrite

Conditions	Yield
With ammonia In water High Pressure; soln. of nitrates, adjustment of pH to 8.90 (ammonia), heating at 164°C for 2 h (microwaves); centrifugation, washing; powder X-ray diffraction;	90%
With ammonia In water High Pressure; soln. of nitrates, adjustment of pH to 8.66 (ammonia), heating at 192°C for 2 h (microwaves); centrifugation, washing; powder X-ray diffraction;	83%
With formaldehyd; triethylamine In water byproducts: (CH2)6N4, H2O, {(C2H5)3NH}NO3; addn. of polyvinyl alcohol to metal nitrate soln., heated with stirring, addn. of mixt. of (NH4)2CO3 or NH4HCO3, triethylamine and formaline to soln., warmed, pptn. (10-12 h); filtered, washed, dried in an oven, heated (1000°C, 8-10 h), XRD, EDX;

bismuth(III) nitrate + oxalic acid (144-62-7) + ferric nitrate (7782-61-8) → bismuth ferrite

Conditions	Yield
In nitric acid Bi(NO3)3 and Fe(NO3)3 dissolved in 2N nitric acid, oxalic acid added under stirring, heated to boiling temp., evapd., dried at 130°C for 30 min, calcined at 600°C for 2 h; XRD, SEM, TG/DTA;	90%

2,6-pyridinedihexanoic acid hydrochloride (1227848-19-2) + water (7732-18-5) + ferric nitrate (7782-61-8) → [Fe3(μ3-O)(2,6-pyridinedihexanoic acid(-H))3]Cl[NO3]3*7H2O

Conditions	Yield
With LiOH In methanol N2; ligand hydrochloride (1 equiv.) and LiOH (2 equiv.) stirred in MeOH for 20 min, evapd., dissolved (MeOH), Fe(NO3)3 (1 equiv.) added dropwise, stirred for 5 min; filtered off, elem. anal.;	90%

ortho-nitrobenzoic acid (552-16-9) + ferric nitrate (7782-61-8) → iron(III) o-nitrobenzoate

Conditions	Yield
With sodium dodecylsulfonate In ethanol; water Fe-compd. and o-nitrobenzoic acid dissolved in ethanol-water (5:1) solution respectively, two solution mixed, sodium dodecylsulfonate added, pH ajusted slowly to 2.7 with stirring, aged for 8 h; filtered, washed with ethanol-water (5:1), dried in air at 80°C;	89%

3-phenylpentane-2,4-dione (5910-25-8) + ferric nitrate (7782-61-8) → tris(3-phenylacetylacetonato)iron(III)

Conditions	Yield
With NaHCO3 In methanol; water solid NaHCO3 was added during 20 min to a well-stirred soln. 3-(4-pyridyl)pentane-2,4-dione in CH3OH and H2O, the mixt. was combined with a soln. of Fe-salt in H2O; ppt. was dissolved in dry methanol, slow evapd.;	88%

N-(5-sulphonyl-8-hydroxyquinoline)-3,5-dimethyl-2-pyrazoline 5-one (136950-29-3) + ferric nitrate (7782-61-8) → Fe(C14H12N3O3S)2(1+)*NO3(1-) = Fe(C14H12N3O3S)2NO3

Conditions	Yield
In ethanol refluxing org. ligand and Fe(NO3)3 (molar ratio 2:1) with stirring at 50-60°C, pptn.; filtration, washing (alcohol), drying; elem. anal.;	87%

zinc(II) nitrate (10196-18-6) + ferric nitrate (7782-61-8) → zinc ferrite

Conditions	Yield
With ammonia In water High Pressure; soln. of nitrates, adjustment of pH to 8.03 (ammonia), heating at 192°C for 2 h (microwaves); centrifugation, washing; powder X-ray diffraction;	86%
With ammonia In water High Pressure; soln. of nitrates, adjustment of pH to 8.05 (ammonia), heating at 164°C for 2 h or 4 mins. (microwaves); centrifugation, washing; powder X-ray diffraction;	84%
In water High Pressure; rapid expansion of supercritical mixed soln. of Zn(NO3)2 and Fe(NO3)3 (100 MPa, 773 K, dwelling time of 6-7 s, concn. of 0.05 M, pH 1.5), isothermal 1-h anneal at temp. from the range of 823-873 K; SEM, TEM, X-ray diffraction anals.;	30%

5-<3'-methyl-5'-oxo-4',5'-dihydropyrazol-1-yl-sulfonyl>-8-quinolinol (136950-28-2) + ferric nitrate (7782-61-8) → Fe(C13H10N3O4S)2(1+)*NO3(1-) = Fe(C13H10N3O4S)2NO3

Conditions	Yield
In ethanol refluxing org. ligand and Fe(NO3)3 (molar ratio 2:1) with stirring at 50-60°C, pptn.; filtration, washing (alcohol), drying; elem. anal.;	84%

potassium tellurite hydrate + ferric nitrate (7782-61-8) → 4Fe(3+)*3Te2O5(2-)*6OH(1-)*8H2O=Fe2(Te2O5)3*2Fe(OH)3*8H2O

Conditions	Yield
In ethanol; water aq. Te-salt soln. in min. solvent addn. to metal salt soln. (EtOH), mixt. stirring for 2 h; ppt. filtration, washing (water, EtOH), air drying; elem. anal.;	83.4%

3-(pyridin-4-yl)-1-diethylaminopentane + ferric nitrate (7782-61-8) → 5-diethylamino-3-pyridin-4-yl-pentan-1-ol (26684-72-0)

Conditions	Yield
With ammonium chloride In ammonia	83%

water (7732-18-5) + ferric nitrate (7782-61-8) + N,N'-bis[1,3-benzodioxol-5-ylmethylene]ethane-1,2-diamine (101732-00-7) → Fe(N,N'-bis[1,3-benzodioxol-5-ylmethylene]ethane-1,2-diamine)(NO3)3(H2O) (1231901-00-0)

Conditions	Yield
In methanol; water Fe-compd. dissolved in CH3OH-H2O, added to refluxing diamine-compd. in CH3OH (molar ratio Fe-diamine=1:1), refluxed for 2 to 3 h; concentrated, washed with Et2O and petroleum ether, filtered, washed with suitable solvents, dried over anhydrous CaCl2, elem. anal.;	82%

2poap (263552-39-2) + water (7732-18-5) + ferric nitrate (7782-61-8) → Fe9(NC5H3(C(O)N2C(NH2)C5H4N)2)6(15+)*15NO3(1-)*19H2O=[Fe9(NC5H3(C(O)N2C(NH2)C5H4N)2)6](NO3)15*19H2O

Conditions	Yield
In water the ligand added to a hot soln. of metal salt; filtered, stand at room temp. for several d; elem. anal.;	81%

N-(5-sulphonyl-8-hydroxyquinoline)-3-amino-2-pyrazoline 5-one (136950-27-1) + ferric nitrate (7782-61-8) → Fe(C12H9N4O4S)2(1+)*NO3(1-) = Fe(C12H9N4O4S)2NO3

Conditions	Yield
In ethanol refluxing org. ligand and Fe(NO3)3 (molar ratio 2:1) with stirring at 50-60°C, pptn.;; filtration, washing (alcohol), drying; elem. anal.;;	80%

imidotetraphenyldiphosphinic acid (31239-06-2) + ferric nitrate (7782-61-8) → Fe((OP(C6H5)2)2N)3

Conditions	Yield
In ethanol refluxing for 2 h; vol. reduction (pptn.);	80%

Upstream product

• 7697-37-2 nitric acid 
• 7439-89-6 iron 
• 13463-40-6 iron pentacarbonyl 

Downstream Products

• 7439-89-6 iron 
• 2338-05-8 ferric citrate 
• 130645-18-0 4,4'-Bis(2-phenylethyl)-6,6'-dimethyl-2,2'-bipyridine 
• 6261-22-9 pent-2-yn-1-ol 
• 764-60-3 hex-2-yn-1-ol 
• 26684-57-1 3-[4]pyridyl-pentane-1,5-diol 
• 26684-56-0 4-(tetrahydro-2H-pyran-4-yl)pyridine 
• 35249-89-9 ammonium glycolate 
• 15377-81-8 hexaaquairon(III) 
• 7439-89-6 iron(II) 
• 10102-44-0 Nitrogen dioxide 
• 1345-25-1 iron(II) oxide 
• 7553-56-2 iodine 
• 7705-08-0 iron(III) chloride 

Relevant articles and documents

Environmentally Benign Solution-Based Procedure for the Fabrication of Metal Oxide Coatings on Metallic Pigments

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

IRON/SHIKONIN NANO-COMPOSITE AND USE THEREOF AND METHOD FOR PREPARING THE SAME BY SUPERMOLECULAR SELF-ASSEMBLY

An iron/shikonin nano-composite and a use thereof, and a method for preparing the same by supermolecular self-assembly, belonging to the technical field of functional materials. The composite consists of shikonin and ferric ions, wherein shikonin is coordinated with the ferric ions, and the hydroxyl and carbonyl groups in shikonin are coordinated with the ferric irons to form a complex, which is then assembled by π-π stacking and hydrophobic interactions to form a nano-composite which exhibits glutathione response. The composite is obtained by the following steps: adding an aqueous solution of a ferric salt and an organic solvent solution of shikonin in sequence into water while stirring at ambient temperature, continuously stirring at ambient temperature, and centrifuging the resulting mixture to purify, thereby obtaining an iron/shikonin nano-composite in the resulting solution.

The kinetics of hydrochemical oxidation of iron(II) persulfide (pyrite) by nitric acid

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.

The Kinetics of Formation of Chromium(III) and Iron(III) Polynuclear Hydroxo Complexes in Nitrate Solutions

The kinetics of Cr3+, Fe3+, and Cr3+-Fe3+ hydrolysis in nitrate solutions at various temperatures is studied by spectrophotometry and potentiometry. The kinetic parameters of formation of polynuclear hydroxo complexes in the systems are determined by using the transformation coefficients.

Investigation of montmorillonite-based clays in the preparation of supported ferric nitrate

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.

Enzymatic oxidation of glycolic acid in the presence of non-enzymatic catalyst for decomposing hydrogen peroxide

A process for the production of glyoxylic acid by reacting glycolic acid and oxygen in an aqueous solution at pH 7-10 in the presence of the enzyme glycolate oxidase and a non-enzymatic catalyst for the decomposition of hydrogen peroxide, and an amine buffer capable of forming a chemical adduct with glyoxylic acid.

5,6,7-Trinor-4,8-inter-m-phenylene prostaglandin I2 derivatives useful in anti-ulcer, hypotensive and platelet aggregation inhibiting compositions

A compound of the formula STR1 wherein R1 is a pharmaceutically acceptable cation, hydrogen or n-alkyl of 1 to 12 carbon atoms; R2 is hydrogen, acyl of 2 to 10 carbon atoms or aroyl of 7 to 13 carbon atoms; R3 is hydrogen, acyl of 2 to 10 carbon atoms or aroyl of 7 to 13 carbon atoms; R4 is hydrogen, methyl or ethyl; R5 is n-alkyl of 1 to 5 carbon atoms; n is an integer of 0 to 4; A is --CH2 --CH2 -- or trans --CH=CH--; and X is --CH2 --CH2 -- or trans --CH=CH--. The compounds are useful in anti-ulcer, hypotensive and platelet aggregation inhibiting compositions.

Process for producing p-xylene

In a process for producing p-xylene which comprises catalytically methylating toluene with a methylating agent in the gaseous phase, the improvement wherein (a) said methylation is carried out continuously in a multi-stage reaction system consisting of a plurality of separate series-connected fixed catalyst layers without separating the resulting xylenes in an intermediate stage, (b) said toluene is fed together with hydrogen gas into only the first-stage fixed catalyst layer and passed successively through the subsequent fixed catalyst layers, the amount of toluene fed being such that the total weight hourly space velocity of toluene is from 1 to 300 hr-1, (c) said methylating agent is fed into each of said fixed catalyst layers, if desired together with hydrogen gas, the amount of the methylating agent fed into each catalyst layer being 0.01/t moles to 1/t moles, in which t is the number of methyl groups in the methylating agent, per mole of toluene fed into the first-stage catalyst layer, and the total amount of the methylating agent fed into all of the catalyst layers being within the range of 0.1/t moles to 2/t moles, in which t is as defined, per mole of toluene fed into the first-stage catalyst layer, and (d) each fixed catalyst layer is filled with a catalyst composed of a crystalline aluminosilicate containing magnesium oxide or lanthanide oxide.