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6047-25-2

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6047-25-2 Usage

Description

Iron(II) oxalate, FeC204.2H20, is precipitated as yellow crystals from solutions containing iron(II) and oxalate ions ; in the presence of excess alkali metal oxalate, however, soluble oxalato complexes M2[Fe(C2O4)2] are formed which can be precipitated by the addition of alcohol. The oxalate is paramagnetic with μeff= 5·2 B.M. at room temperature.

Chemical Properties

yellow powder Ferrous oxalate, or iron(II) oxalate, is a chemical compound consisting of one iron(II) ion (Fe2) and one oxalate ion (C2O4(2?)). It has the chemical formula FeC2O4. Iron(II) oxalate is more commonly encountered as the dihydrate, FeC2O4·2H2O, CAS # 6047-25-2. Its crystal structure consists of chains of oxalate-bridged iron atoms, capped by water molecules. When heated, it dehydrates and decomposes into carbon dioxide, carbon monoxide, iron oxides and pyrophoric black iron.

Uses

It is used as photographic developer for silver bromide-gelatin plates. It imparts greenish-brown tint to optical glass (sunglasses, windshields, railroad car windows), for decorative glassware, pigment for plastics, paints and lacquers. It acts as reagent.

Check Digit Verification of cas no

The CAS Registry Mumber 6047-25-2 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 6,0,4 and 7 respectively; the second part has 2 digits, 2 and 5 respectively.
Calculate Digit Verification of CAS Registry Number 6047-25:
(6*6)+(5*0)+(4*4)+(3*7)+(2*2)+(1*5)=82
82 % 10 = 2
So 6047-25-2 is a valid CAS Registry Number.
InChI:InChI=1/C2H2O4.Fe.2H2O/c3-1(4)2(5)6;;;/h(H,3,4)(H,5,6);;2*1H2/q;+2;;/p-2

6047-25-2 Well-known Company Product Price

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  • Alfa Aesar

  • (10718)  Iron(II) oxalate dihydrate, Puratronic?, 99.999% (metals basis)   

  • 6047-25-2

  • 2.5g

  • 228.0CNY

  • Detail
  • Alfa Aesar

  • (10718)  Iron(II) oxalate dihydrate, Puratronic?, 99.999% (metals basis)   

  • 6047-25-2

  • 25g

  • 549.0CNY

  • Detail
  • Alfa Aesar

  • (10718)  Iron(II) oxalate dihydrate, Puratronic?, 99.999% (metals basis)   

  • 6047-25-2

  • 100g

  • 1121.0CNY

  • Detail
  • Alfa Aesar

  • (10718)  Iron(II) oxalate dihydrate, Puratronic?, 99.999% (metals basis)   

  • 6047-25-2

  • 500g

  • 4915.0CNY

  • Detail
  • Alfa Aesar

  • (A13479)  Iron(II) oxalate dihydrate, 99%   

  • 6047-25-2

  • 250g

  • 407.0CNY

  • Detail
  • Alfa Aesar

  • (A13479)  Iron(II) oxalate dihydrate, 99%   

  • 6047-25-2

  • 1000g

  • 1443.0CNY

  • Detail
  • Aldrich

  • (255971)  Iron(II)oxalatedihydrate  ≥99.99% trace metals basis

  • 6047-25-2

  • 255971-10G

  • 556.92CNY

  • Detail
  • Aldrich

  • (307726)  Iron(II)oxalatedihydrate  99%

  • 6047-25-2

  • 307726-25G

  • 391.95CNY

  • Detail
  • Aldrich

  • (307726)  Iron(II)oxalatedihydrate  99%

  • 6047-25-2

  • 307726-500G

  • 563.94CNY

  • Detail

6047-25-2SDS

SAFETY DATA SHEETS

According to Globally Harmonized System of Classification and Labelling of Chemicals (GHS) - Sixth revised edition

Version: 1.0

Creation Date: Aug 18, 2017

Revision Date: Aug 18, 2017

1.Identification

1.1 GHS Product identifier

Product name Ferrous oxalate dihydrate

1.2 Other means of identification

Product number -
Other names Eisen(II)-oxalat-dihydrat

1.3 Recommended use of the chemical and restrictions on use

Identified uses For industry use only.
Uses advised against no data available

1.4 Supplier's details

1.5 Emergency phone number

Emergency phone number -
Service hours Monday to Friday, 9am-5pm (Standard time zone: UTC/GMT +8 hours).

More Details:6047-25-2 SDS

6047-25-2Synthetic route

oxalic acid hydrazide
996-98-5

oxalic acid hydrazide

iron(II) sulfate pentahydrate

iron(II) sulfate pentahydrate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water at 135℃; for 24h; Temperature;95.3%
oxalic acid hydrazide
996-98-5

oxalic acid hydrazide

water
7732-18-5

water

iron(II) chloride

iron(II) chloride

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
at 150℃; for 15h;94.8%
iron(III) chloride hexahydrate

iron(III) chloride hexahydrate

sodium oxalate
62-76-0

sodium oxalate

A

iron(II,III) oxide

iron(II,III) oxide

B

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water autoclave (160°C, 16 h); cooling to room temp. over 4 h, filtration, drying in air, removal of some magnetite with the help of a bar magnet;A n/a
B 68%
potassium ferrioxalate

potassium ferrioxalate

water
7732-18-5

water

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
With nicotinic acid In water High Pressure; under hydrothermal conditions; Fe complex, nicotinic acid and H2O (molarratio 1:2:1100) in stailess steel vessel heated at 160°C for 3 d; filtered; crystals washed with distd. H2O; dried in air at ambient temp.; elem. anal.;50%
sodium oxalate
62-76-0

sodium oxalate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
With water; iron(II) sulfate; Petroleum ether
potassium oxalate
583-52-8

potassium oxalate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
With iron (II)-ammonium sulfate
oxalic acid
144-62-7

oxalic acid

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
With iron(II) sulfate
iron(III) oxide

iron(III) oxide

oxalic acid
144-62-7

oxalic acid

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water autoclave (220°C, 40 h); slow cooling to room temp. over 3-4 h;
sodium oxalate
62-76-0

sodium oxalate

iron(III) chloride
7705-08-0

iron(III) chloride

A

iron(II,III) oxide

iron(II,III) oxide

B

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water autoclave (160-200°C, 16-19 h); slow cooling to room temp. over 3-4 h;
sodium oxalate
62-76-0

sodium oxalate

iron(II) chloride

iron(II) chloride

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water autoclave (180°C, 96 h); slow cooling to room temp. over 3-4 h;
iron(III) chloride
7705-08-0

iron(III) chloride

disodium oxomalonate

disodium oxomalonate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
With NaCl In water autoclave (160°C, 68 h); slow cooling to room temp. over 3-4 h;
oxalic acid
144-62-7

oxalic acid

iron(II) sulfate

iron(II) sulfate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water; glycerol stirring at 320 K; washed with hot water, dried;
In water pptn. on mixing components solns.; ppt. filtration, washing and drying;
In water prepn. by adding a twofold stoich. excess of hot (70°C) soln. of oxalic acid to aq. soln. of metal salt under stirring for 60 min; ppt. allowed to ripen for 12 h; filtered; washed (H2O); dried under ambient conditions;
iron(II) sulfate

iron(II) sulfate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
With oxalic acid In water pptn.; filtration, washing, drying;
ammonium trioxalatoferrate(III) trihydrate

ammonium trioxalatoferrate(III) trihydrate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In neat (no solvent, solid phase) Irradiation (UV/VIS); solid state photolysis in visible region at 25°C for 100-200 h; not isolated, detected by Moessbauer spectroscopy;
iron(II) chloride tetrahydrate

iron(II) chloride tetrahydrate

oxalic acid
144-62-7

oxalic acid

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In ethanol; water Fe-salt dissoln. (mixed solvent with small amt. of HCl to prevent Fe(II)oxidn.), pptn. at 20°C on org. acid soln. (EtOH) addn., stirring for 5 min; ppt. filtration, washing (water), drying at 90°C; XRD, SEM;
In N,N-dimethyl acetamide; water for 0.0833333h;
lithium tris(oxalato)ferrate(III) trihydrate

lithium tris(oxalato)ferrate(III) trihydrate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In neat (no solvent, solid phase) Irradiation (UV/VIS); solid state photolysis in visible region at 25°C for 100-200 h; not isolated, detected by Moessbauer spectroscopy;
iron sulfide

iron sulfide

ammonium oxalate

ammonium oxalate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In not given
In not given
oxalic acid
144-62-7

oxalic acid

iron(III) chloride
7705-08-0

iron(III) chloride

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water Irradiation (UV/VIS); calm standing for several months (weak admission of light);;
In water Irradiation (UV/VIS); calm standing for several months (weak admission of light);;
ammonium oxalate

ammonium oxalate

iron(III) chloride
7705-08-0

iron(III) chloride

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water Irradiation (UV/VIS); intensive irradiation causes fast reaction;;
In water Irradiation (UV/VIS); calm standing for several months (weak admission of light);;
In water Irradiation (UV/VIS); intensive irradiation causes fast reaction;;
In water Irradiation (UV/VIS); calm standing for several months (weak admission of light);;
ferrous(II) sulfate heptahydrate

ferrous(II) sulfate heptahydrate

oxalic acid
144-62-7

oxalic acid

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water FeC2O4*2H2O dissolved in bidistd. H2O, oxalic acid added till complete pptn.; ppt. filtered washed with distd. H2O, dried;
In water to aq.-soln. of FeSO4*7H2O soln. of oxalic acid added, stirred until pptn.; ppt. filtered, washed with distd. water dried in air;
ferrous(II) sulfate heptahydrate

ferrous(II) sulfate heptahydrate

ammonium oxalate monohydrate
6009-70-7

ammonium oxalate monohydrate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
copptn. at 60°C; ppt. washing (water, alcohol, acetone), drying at ca. 80°C; DSC;
iron(II) nitrate

iron(II) nitrate

potassium oxalate
583-52-8

potassium oxalate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water mixing (ambient temp.); nucleation rate and mechanism investigated;
oxalate dianion
338-70-5

oxalate dianion

iron(II)
7439-89-6

iron(II)

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water pptn. of iron(II) salt soln. by alkali oxalate (at 30 °C or boiling soln.);;
In water pptn. of iron(II) salt soln. by alkali oxalate; sepn. within several hours;; dried up to 100 °C; impurities of alkali;;
In water pptn. of iron(II) salt soln. by alkali oxalate;; dried at higher temperatures;;
oxalic acid
144-62-7

oxalic acid

iron(II)
7439-89-6

iron(II)

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water pptn. of iron(II) salt soln. (at 30 °C or boiling soln.);;
In water pptn. of iron(II) salt soln.; sepn. within several hours;; dried up to 100 °C;;
In water pptn. of iron(II) salt soln.;; dried at higher temperatures;;
oxalic acid
144-62-7

oxalic acid

iron(II) chloride

iron(II) chloride

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In not given
ferrous ammonium sulphate

ferrous ammonium sulphate

potassium oxalate
583-52-8

potassium oxalate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water pptn. from dilute aq. soln. of (NH4)2Fe(SO4)2 and soln. of K2C2O4 under N2;
In water aq. (NH4)2Fe(SO4)2 titrated with aq. K2C2O4 to pH 7 at 298 K; filtered, washed (H2O), vacuum-dried for 24 h; XRD;
potassium oxalate
583-52-8

potassium oxalate

iron(II) sulfate

iron(II) sulfate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water pptn. from metal sulphate soln. with K-salt soln.; XRD;
ferric oxalate
15843-42-2

ferric oxalate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water Irradiation (UV/VIS); calm standing of concd. soln. for several months (weak admission of light);;
In water Irradiation (UV/VIS); intensive irradiation causes fast reaction;;
In water Irradiation (UV/VIS); intensive irradiation causes fast reaction;;
In water Irradiation (UV/VIS); calm standing of concd. soln. for several months (weak admission of light);;
ammonium oxalate

ammonium oxalate

iron(II)
7439-89-6

iron(II)

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
In water pptn. of iron(II) salt soln. by ammonium oxalate; sepn. within several hours;; dried up to 100 °C;;
In water pptn. of iron(II) salt soln. by ammonium oxalate; sepn. within several hours;; dried up to 100 °C;;
ammonium oxalate

ammonium oxalate

iron(II) sulfate

iron(II) sulfate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Conditions
ConditionsYield
components copptn. at 60°C; ppt. washing (water, acetone), drying at 80°C; DSC;
trifluorormethanesulfonic acid
1493-13-6

trifluorormethanesulfonic acid

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

2,3,11,12-dibenzo-1,4,7,10,13,16-hexathia-cyclooctadeca-2,11-diene
105400-44-0

2,3,11,12-dibenzo-1,4,7,10,13,16-hexathia-cyclooctadeca-2,11-diene

(2,3,11,12-dibenzo-1,4,7,10,13,16-hexathiacyclooctadeca-2,11-diene)Fe(trifluoromethanesulfonate)2*dioxane

(2,3,11,12-dibenzo-1,4,7,10,13,16-hexathiacyclooctadeca-2,11-diene)Fe(trifluoromethanesulfonate)2*dioxane

Conditions
ConditionsYield
With dioxane In 1,4-dioxane N2 atmosphere; refluxing (1 h); filtration, washing (dioxane), drying (vac.); elem. anal.;91%
barium bromide dihydrate

barium bromide dihydrate

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

Ba4[Fe(μ3-OH)6(C2O4)6]Br2*6H2O

Ba4[Fe(μ3-OH)6(C2O4)6]Br2*6H2O

Conditions
ConditionsYield
With pyridine-2,6-dicarboxylic acid In water High Pressure; heated at 473 K for 72 h in an autoclave; cooled to room temp., crystals isolated, washed (H2O), dried (air); elem. anal.;86%
thorium tetrafluoride
13709-59-6

thorium tetrafluoride

hydrogen fluoride
7664-39-3

hydrogen fluoride

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

sodium fluoride

sodium fluoride

Na3FeTh6F30

Na3FeTh6F30

Conditions
ConditionsYield
In water at 200℃; for 36h; Time; Autoclave; High pressure;83%
erbium(III) chloride hexahydrate

erbium(III) chloride hexahydrate

phosphonomethylimino-di-acetic acid
5994-61-6

phosphonomethylimino-di-acetic acid

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

[ErFe(III)(Fe(II))6(N-(phosphonomethyl)iminodiacetateH)6]*nH2O

[ErFe(III)(Fe(II))6(N-(phosphonomethyl)iminodiacetateH)6]*nH2O

Conditions
ConditionsYield
With aq. NaOH In further solvent(s) to mixt. of acid, Fe oxalate, ErCl3*6H2O added eutectic mixt. of cholinechloride and malonic acid and aq. NaOH; suspn. magnetically stirred for 1 h at ambient temp.; gel transferred to react. vessel, placed in prehe ated oven (at 150°C) for 90 h; washed 3 times with EtOH with ultrasonic vibration and with water; air dried at ambient temp.;76%
vanadia

vanadia

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

A

iron(III) oxide

iron(III) oxide

B

barium divanadate

barium divanadate

BaNa1.63Fe0.79[VO4]2

BaNa1.63Fe0.79[VO4]2

Conditions
ConditionsYield
Stage #1: vanadia; iron(II) oxalate dihydrate With sodium carbonate; barium carbonate at 499.84℃; for 3h; Inert atmosphere;
Stage #2: for 36h; Heating;
A 4%
B 20%
C 76%
iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

molybdic acid

molybdic acid

ethylenediamine
107-15-3

ethylenediamine

NH3CH2CH2NH3(2+)*Fe(2+)*C2O4(2-)*MoO4(2-)=NH3CH2CH2NH3Fe(C2O4)MoO4

NH3CH2CH2NH3(2+)*Fe(2+)*C2O4(2-)*MoO4(2-)=NH3CH2CH2NH3Fe(C2O4)MoO4

Conditions
ConditionsYield
In water mixt. of Fe(C2O4)*2H2O, molybic acid and ethylenediamine was sealed with H2O in tube, heated at 100°C for 24 h; washed with acetone and ether;75%
4,4'-bipyridine
553-26-4

4,4'-bipyridine

hydrogen fluoride
7664-39-3

hydrogen fluoride

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

orthoarsenic acid
7778-39-4, 121471-47-4

orthoarsenic acid

[4,4'-bpyH2]3[Fe9(H2O)6F3(HAsO4)12(AsO4)2]*2H2O

[4,4'-bpyH2]3[Fe9(H2O)6F3(HAsO4)12(AsO4)2]*2H2O

Conditions
ConditionsYield
In water High Pressure; stainless steel acid-digestion vessel, aq. H3AsO4 was added to a mixt. of Fe-compd. and N-compd., 48 % aq. HF was added, room temp., 30 min stirring (Fe:As:bipyridine:HF:H2O molar ratio was 1:8:4:6:200), 150 and 170 °C for 72 and 24 h, resp.; crystals were filtered off, washed with H2O, dried at ambient temp., elem. anal.;75%
trifluorormethanesulfonic acid
1493-13-6

trifluorormethanesulfonic acid

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

2,3,11,12-dibenzo-1,4,7,10,13,16-hexathia-cyclooctadeca-2,11-diene
105400-44-0

2,3,11,12-dibenzo-1,4,7,10,13,16-hexathia-cyclooctadeca-2,11-diene

(2,3,11,12-dibenzo-1,4,7,10,13,16-hexathiacyclooctadeca-2,11-diene)Fe(trifluoromethanesulfonate)2

(2,3,11,12-dibenzo-1,4,7,10,13,16-hexathiacyclooctadeca-2,11-diene)Fe(trifluoromethanesulfonate)2

Conditions
ConditionsYield
In further solvent(s) N2 atmosphere; refluxing in EtNO2 (1 h), cooling (room temp.); filtration, cooling (-30°C, overnight), washing (THF), drying (vac.); elem. anal.;66%
phosphonomethylimino-di-acetic acid
5994-61-6

phosphonomethylimino-di-acetic acid

europium(III) chloride hexahydrate

europium(III) chloride hexahydrate

water
7732-18-5

water

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

[EuFeFe6(N-(phosphonomethyl)iminodiacetic acid-3H)6]·2H2O

[EuFeFe6(N-(phosphonomethyl)iminodiacetic acid-3H)6]·2H2O

Conditions
ConditionsYield
With malonic acid; choline chloride; sodium hydroxide at 150℃; for 72h; Autoclave; High pressure;63%
iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

molybdic acid

molybdic acid

ethylenediamine
107-15-3

ethylenediamine

A

NH2CH2CH2NH2*Fe(2+)*MoO4(2-)=NH2CH2CH2NH2FeMoO4

NH2CH2CH2NH2*Fe(2+)*MoO4(2-)=NH2CH2CH2NH2FeMoO4

B

NH3CH2CH2NH3(2+)*Fe(2+)*C2O4(2-)*MoO4(2-)=NH3CH2CH2NH3Fe(C2O4)MoO4

NH3CH2CH2NH3(2+)*Fe(2+)*C2O4(2-)*MoO4(2-)=NH3CH2CH2NH3Fe(C2O4)MoO4

Conditions
ConditionsYield
In water mixt. of Fe(C2O4)*2H2O, molybic acid and ethylenediamine was sealed with H2O in tube, heated at 100°C for 24 h; washed with acetone and ether;A 57%
B 2%
iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

sodium benzene-1,2,4,5-tetracarboxylate
148-04-9

sodium benzene-1,2,4,5-tetracarboxylate

Fe2(μ8-benzene-1,2,4,5-tetracarboxylate)(μ2-oxalate)*(H3O)2(H2O)2

Fe2(μ8-benzene-1,2,4,5-tetracarboxylate)(μ2-oxalate)*(H3O)2(H2O)2

Conditions
ConditionsYield
In water High Pressure; FeC2O4*2H2O, Na2C2O4*2H2O, Na4bta and H2O were placed in stainless steelvessel, heated at 160°C for 5 d under autogenous pressure, coole d to room temp.; filtered, purified by repeated cycles of treating aq. slurry in ultrasonic bath; elem. anal.;56%
1,2,4-Triazole
288-88-0

1,2,4-Triazole

water
7732-18-5

water

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

[Fe2(H2O)(oxalate)][Fe2(1,2,4-triazole(-1H))6]*2.5H2O

[Fe2(H2O)(oxalate)][Fe2(1,2,4-triazole(-1H))6]*2.5H2O

Conditions
ConditionsYield
With sodium fluoride at 180℃; for 168h; High pressure;56%
phosphonomethylimino-di-acetic acid
5994-61-6

phosphonomethylimino-di-acetic acid

holmium(III) chloride hexahydrate

holmium(III) chloride hexahydrate

water
7732-18-5

water

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

[HoFeFe6(N-(phosphonomethyl)iminodiacetic acid-3H)6]·2H2O

[HoFeFe6(N-(phosphonomethyl)iminodiacetic acid-3H)6]·2H2O

Conditions
ConditionsYield
With malonic acid; choline chloride; sodium hydroxide at 150℃; for 72h; Autoclave; High pressure;56%
gadolinium(III) chloride hexahydrate

gadolinium(III) chloride hexahydrate

phosphonomethylimino-di-acetic acid
5994-61-6

phosphonomethylimino-di-acetic acid

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

[GdFe(III)(Fe(II))6(N-(phosphonomethyl)iminodiacetateH)6]*nH2O

[GdFe(III)(Fe(II))6(N-(phosphonomethyl)iminodiacetateH)6]*nH2O

Conditions
ConditionsYield
With aq. NaOH In further solvent(s) to mixt. of acid, Fe oxalate, GdCl3*6H2O added eutectic mixt. of cholinechloride and malonic acid and aq. NaOH; suspn. magnetically stirred for 1 h at ambient temp.; gel transferred to react. vessel, placed in prehe ated oven (at 150°C) for 90 h; washed 3 times with EtOH with ultrasonic vibration and with water; air dried at ambient temp.;51%
piperazine
110-85-0

piperazine

hydrogen fluoride
7664-39-3

hydrogen fluoride

water
7732-18-5

water

iron(II) oxalate dihydrate
6047-25-2

iron(II) oxalate dihydrate

orthoarsenic acid
7778-39-4, 121471-47-4

orthoarsenic acid

[piperazinium]1.5[Fe3(HAsO4)2(AsO4)F5]

[piperazinium]1.5[Fe3(HAsO4)2(AsO4)F5]

Conditions
ConditionsYield
In water High Pressure; mixt. of Fe(C2O4)*2H2O:H3AsO4:piperazine:HF:H2O = 1:8:4:6:200 heated at 150°C for 168 h or at 180°C for 24 h, in a PTFE-lined aciddigestion bomb;50%

6047-25-2Relevant articles and documents

Concerning the cation distribution in MnFe2O4 synthesized through the thermal decomposition of oxalates

Gabal,Ata-Allah

, p. 995 - 1003 (2004)

A single phase manganese ferrite powder have been synthesized through the thermal decomposition reaction of MnC2O4·2H 2O-FeC2O4·2H2O (1:2 mole ratio) mixture in air. DTA-TG, XRD, Mo?ssbauer spectroscopy, FT-IR and SEM techniques were used to investigate the effect of calcination temperature on the mixture. Firing of the mixture in the range 300-500 °C produce ultra-fine particles of α-Fe2O3 having paramagnetic properties. XRD, Mo?ssbauer spectroscopy as well as SEM experiments showed the progressive increase in the particle size of α-Fe2O 3 up to 500 °C. DTA study reveals an exothermic phase transition at 550 °C attributed to the formation of a Fe2O 3-Mn2O3 solid solution which persists to appear up to 1000 °C. At 1100 °C, the single phase MnFe 2O4 with a cubic structure predominated. The Mo?ssbauer effect spectrum of the produced ferrite exhibits normal Zeeman split sextets due to Fe3+ions at tetrahedral (A) and octahedral (B) sites. The obtained cation distribution from Mo?ssbauer spectroscopy is (Fe0.92Mn0.08)[Fe1.08Mn0.92]O 4.

Cation-substituted LiFePO4 prepared from the FeSO4·7H2O waste slag as a potential Li battery cathode material

Wu, Ling,Wang, Zhixing,Li, Xinhai,Guo, Huajun,Li, Lingjun,Wang, Xiaojuan,Zheng, Junchao

, p. 278 - 284 (2010)

The purpose of this study is to utilize the huge FeSO4·7H2O waste slag produced by the titanium dioxide industry. FeC2O4·2H2O precursors are synthesized at various pH values by using the waste slag and H2C2O4·2H2O as raw materials, and without any purifying process. ICP analysis confirms that the impurity content of FeC2O4·2H2O increases with the pH value. Crystalline cation-substituted LiFePO4 are prepared from the FeC2O4·2H2O precursors. The cation dopants do not obviously change the structure of LiFePO4, and all the samples are single olivine-type phase and well crystallized. The lattice parameters of LiFePO4 decrease with the increased dopants contents. The dopants limit the size of LiFePO4 nanocrystals, LiFePO4 particles agglomeration and, consequently, improve the electrochemical performance of LiFePO4. The cation-substituted LiFePO4 prepared from the waste slag show much better electrochemical properties than the pure LiFePO4 at high current rates. The optimal pH value for synthesizing FeC2O4·2H2O from the waste slag is about 1.0, with 96.6% iron recovery. The cation-substituted LiFePO4 prepared from this precursor exhibits the best electrochemical properties, which delivers a capacity of 152, 142 and 126 mAh g-1 at 1C, 2C and 5C rate, respectively, and shows excellent cycling performance.

The low temperature synthesis of metal oxides by novel hydrazine method

Rane,Uskaikar,Pednekar,Mhalsikar

, p. 627 - 638 (2007)

The hydroxide, oxalate and citrate precursors of the metal oxides such as γ-Fe2O3, (MnZn)Fe2O4, Cu(K)Fe2O4, BaTiO3, La(Sr)MnO3, La(Sr)AlO3, La/Gd(Ca/Ba/Sr)C

Large-scale fabrication of porous carbon-decorated iron oxide microcuboids from Fe-MOF as high-performance anode materials for lithium-ion batteries

Li, Minchan,Wang, Wenxi,Yang, Mingyang,Lv, Fucong,Cao, Lujie,Tang, Yougen,Sun, Rong,Lu, Zhouguang

, p. 7356 - 7362 (2015)

A facile, cost-effective and environmentally friendly route has been developed to synthesise porous carbon-decorated iron oxides on a large scale via annealing iron metal-organic framework (MOF) precursors. The as-prepared C-Fe3O4 particles exhibit microcuboid-like morphologies that are actually composed of ultrafine nanoparticles and show a greatly enhanced lithium storage performance with high specific capacity, excellent cycling stability and good rate capability. The C-Fe3O4 electrodes demonstrate a high reversible capacity of 975 mA h g-1 after 50 cycles at a current density of 100 mA g-1 and a remarkable rate performance, with capacities of 1124, 1042, 886 and 695 mA h g-1 at current densities of 100, 200, 500 and 1000 mA g-1, respectively. The satisfactory electrochemical performance was attributed to the hierarchical architecture, which benefitted from the synergistic effects of the high conductivity of the carbon matrix, the cuboid-like secondary particles on the microscale, and the ultrafine primary nanoparticles on the nanoscale. This low-cost and simple method provides the possibility to prepare anode materials on a large scale and hence may have great potential applications in energy storage and conversion. This journal is

Local magnetic moments in the (Fe1-xNix)4N (0 ≤ x ≤ 0.6) compounds

Yang, Jinbo,Xue, Desheng,Li, Fashen

, p. 2781 - 2785 (1997)

Moessbauer and magnetic measurements have been performed on the single-phase γ′-Fe4N and (Fe1-xNix)4N compounds. The local magnetic moments of iron and nickel atoms are evaluated by combining hyperfine fields an

Intrinsic and extrinsic proton conductivity in metal-organic frameworks

Tominaka,Cheetham

, p. 54382 - 54387 (2014)

Metal-organic frameworks (MOFs), a new class of solid-state materials, have recently been investigated as proton conductors, but little is known about their mechanisms. Since most of the conductivities reported so far were measured using powder samples, there is uncertainty as to whether they exhibit intrinsic proton transport through frameworks and/or micropores, or extrinsic transport through interparticle phases. Herein, we re-visit ferrous oxalate dihydrate [Fe(ox)(H2O)2] (ox = oxalate anion), which is a dense MOF and recognized as a model system for MOF-based proton conductors. By single-crystal measurements using microelectrodes, we show that protons do not transport through the crystals (-9 S cm-1), but that the conductivity observed in powder samples originates from interparticle phases. This result raises a question as to how general is this phenomenon? We have comprehensively surveyed the literature on solid-state proton conductors and found that large numbers of MOFs, including [Fe(ox)(H2O)2], have a similar activation energy to those of gels and interparticle conductors in classical solid-state materials. This indicates a considerable contribution from interparticle phases towards proton conductivity in MOFs, and single crystal analysis or special methods for powder analysis are clearly necessary to confirm intrinsic conductivity. This journal is

Peculiarities of polythermic decomposition of iron, cobalt and nickel oxalates within pores of photonic crystals based on SiO2 in atmosphere with oxygen lack

Zakharov,Mayorova,Perov

, p. 747 - 750 (2008)

Iron(II), cobalt(II) and nickel(II) oxalates were synthesized as nanofractals inside the voids of the photonic crystals based on SiO2. Guest substances undergone polythermic decomposition within the pores of the photonic crystals in helium atmo

Soft magnetic Fe5C2-Fe3C@C as an electrocatalyst for the hydrogen evolution reaction

Ye, Zhantong,Qie, Yaqin,Fan, Zhipeng,Liu, Yixuan,Shi, Zhan,Yang, Hua

, p. 4636 - 4642 (2019)

Herein, cubic iron carbides encapsulated in an N-doped carbon shell (ICs@NC) were prepared by a simple two-step method. The two-step method included the preparation of iron oxalate dihydrate and the process of calcination with ethylenediamine. By changing the calcination temperature, we could control the type of iron carbide formed. Moreover, the prepared iron carbide@N-doped carbon core-shell particles exhibited regular cubic shapes and soft magnetic properties with high saturation magnetization. More importantly, we investigated the electrocatalytic activity of the iron carbide@N-doped carbon catalysts for the hydrogen evolution reaction (HER). The results show that the Fe5C2-Fe3C@NC catalyst has efficient HER catalytic activity with an overpotential of 209 mV@10 mA cm?2.

Method for synthesizing high-purity ferrous oxalate

-

Paragraph 0037-0038, (2019/11/04)

The invention discloses a method for synthesizing high-purity ferrous oxalate. The method comprises the following steps: (1) fully dissolving a ferrous salt in reverse osmosis water, and carrying outfiltering; (2) preparing an oxalyl dihydrazide solution and carrying out filtering; and 3) mixing the ferrous salt solution with the oxalyl dihydrazine solution, then carrying out a reaction, and subjecting the obtained precipitate to filtering, washing, filtering and drying successively so as to obtain high-purity ferrous oxalate dihydrate. The method of the invention has the beneficial effects that oxalyl dihydrazide is used as a reaction raw material, and can be used both as a reactant and a reducing agent after decomposition so as to achieve the purpose of impurity removal, and impurity removal of oxalyl dihydrazide itself is simple, so the purity of the product is improved; the purity of the synthesized ferrous oxalate dihydrate can reach 99.99%, so the added value of the product is high, and the needs of synthesizing lithium iron phosphate can be met; and the method is simple in synthesis process, mild in reaction conditions, friendly to environment and energy-saving, can realizeindustrial production, and has great application value.

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