IRON (III) SULFATE

FERRIC SULFATE

CAS Number: 10028-22-5
EC Number: 233-072-9
Molecular Weight: 399.88
Molecular Formula: Fe2(SO4)3

Iron(III) sulfate (or ferric sulfate), is a family of inorganic compounds with the formula Fe2(SO4)3(H2O)n. 
A variety of hydrates are known, including the most commonly encountered form of "ferric sulfate". 

Solutions are used in dyeing as a mordant, and as a coagulant for industrial wastes. 
Solutions of ferric sulfate are also used in the processing of aluminum and steel.

Iron (III) Sulfate formula or the ferric sulfate is an inorganic salt with the formula Fe2(SO4)3. 
Iron (III) Sulfate is yellow in colour and is soluble in water. 

The molecule is formed of Fe+3 cation and SO4–2 anion. 
Iron (III) Sulfate is found in a wide variety of minerals but mainly Iron (III) Sulfate is found in marcasite and pyrite. 

Mostly, ferric sulfate is extracted from nature but can also be prepared by treating ferrous sulfate with sulfuric acid at elevated temperature. 
In this article, learn more about the Iron (III) Sulfate formula and Iron (III) Sulfate chemical structure along with Iron (III) Sulfate properties and uses.

Ferric Sulfate or Iron (III) sulfate is a chemical compound that is a yellow crystalline solid or a grayish-white power. 
Iron (III) Sulfate is a salt that is soluble in water; a chemical agent with acidic properties. 

The non-flammable compound is considered toxic, harmful if swallowed, and can cause serious eye damage and skin irritation. 
Iron (III) Sulfate may be corrosive to some metals. 
Primary uses for ferric sulfate are for water purification and as a soil conditioner.

Ferric Sulfate is a toxic, non-flammable chemical compound with the molecular formula Fe2O12S3. 
Iron (III) Sulfate CAS is 10028-22-5. 

The dark brown or yellow chemical agent is produced by the reaction of sulfuric acid and an oxidizing agent. 
Ferric sulfate is used in different fields such as dentistry and dermatology. 

Iron (III) Sulfate is thought to present hemostatic properties by interacting chemically with certain blood proteins. 
Other applications include use as an odor agent, solids separation agent, and as a water treatment chemical. 

Solutions are used as a mordant in dying, and as a coagulant for industrial wastes. 
The compound is also used in the manufacture of pigments, and in pickling baths for aluminum and steel.

The FDA lists ferric sulfate as a direct food substance that is affirmed in the GRAS category (Generally Recognized as Safe). 
The primary hazard is a threat to the environment. 
Immediate steps should be taken to limit Iron (III) Sulfate spread in the environment.

Ferric sulfate is produced on a large scale by adding sulfuric acid and an oxidizing agent (e.g., nitric acid or hydrogen peroxide) to a hot solution of ferrous sulfate. 
Iron (III) Sulfate is used to make iron alums and other ferric compounds.

Ferric sulfate has the molecular formula of Fe2SO4, and Iron (III) Sulfate is a dark brown or yellow chemical agent with acidic properties. 
Iron (III) Sulfate is produced by the reaction of sulfuric acid and an oxidizing agent. 

Iron (III) Sulfate is used in different fields such as dermatology, dentistry and Iron (III) Sulfate is thought to present hemostatic properties by interacting chemically with blood proteins.
1,2 By the FDA, ferric sulfate is a direct food substance affirmed in the GRAS category (Generally Recognized As Safe).

Ferric Sulfate is a red-brown aqueous solution that is typically sold as a 50% or 60% strength solution, on a dry basis. 
Based on ferric iron (Fe+3) contents of 10% and 12% respectively for the two concentrations of liquid ferric sulfate, the formula for dry ferric sulfate would be Fe2(SO4)3•8.8H2O. 
The maximum concentration as ferric iron is approximately 13% in commercial liquid products.

Ferric Salts are used in many different municipal and industrial applications. 
Ferric Salts typically are used in water and wastewater treatment operations as coagulants or flocculants for water clarification, for odor control to minimize hydrogen sulfide release, for phosphorus removal, and as a sludge thickening, conditioning and dewatering agent.

Ferric Sulfate is generally immediately available in most volumes. 
High purity, submicron and nanopowder forms may be considered. 

American Elements produces to many standard grades when applicable, including Mil Spec (military grade); ACS, Reagent and Technical Grade; Food, Agricultural and Pharmaceutical Grade; Optical Grade, USP and EP/BP (European Pharmacopoeia/British Pharmacopoeia) and follows applicable ASTM testing standards. 
Typical and custom packaging is available. 
Additional technical, research and safety (MSDS) information is available as is a Reference Calculator for converting relevant units of measurement.

Experimental Properties of Iron (III) Sulfate:

Physical Description of Iron (III) Sulfate:
Ferric sulfate appears as a yellow crystalline solid or a grayish-white powder. 

The primary hazard is the threat to the environment. 
Immediate steps should be taken to limit Iron (III) Sulfate spread to the environment. 
Iron (III) Sulfate is used for water purification, and as a soil conditioner.

Greyish-white solid, slightly soluble in water; Very hygroscopic.
Commercial product is yellow and contains about 20% water.
Off-white or yellow odorless powder.

Speciation of Iron (III) Sulfate:
The various crystalline forms of Fe2(SO4)3(H2O)n are well-defined, often by X-ray crystallography. 
The nature of the aqueous solutions is often less certain, but aquo-hydroxo complexes such as [Fe(H2O)6]3+ and [Fe(H2O)5(OH)]5+ are often assumed.

Regardless, all such solids and solutions feature ferric ions, each with five unpaired electrons. 
By virtue of this high spin d5 electronic configuration, these ions are paramagnetic and are weak chromophores.

Application of Iron (III) Sulfate:
Convenient, efficient catalyst for the preparation of aromatic esters from the corresponding acids and alcohols.

Uses of Iron (III) Sulfate:
Used in water treatment processes to eliminate the sulfur odour.
Used as an oxidizing agent and solid separation agent.
Used in medicines as astringent and styptic.

Used to make iron salts and pigments, as a coagulant in water purification and sewage treatment, in etching aluminum, in pickling stainless steel and copper, as a mordant in textile dyeing and calico printing, in soil conditioners, as a polymerization catalyst, in the coal conversion process (desulfurization), in the ferric salt leaching process, as a disinfectant, and as a hemostatic agent for endodontic surgery.

The primary use for ferric sulfate is in water and wastewater treatment.

In preparation of iron alums, other iron salts and pigments.
As coagulant in water purification and sewage treatment.

In etching aluminum.
In pickling stainless steel and copper.

As mordant in textile dyeing and calico printing.
In soil conditioners.
As polymerization catalyst.

Industrial Processes with risk of exposure:
Aluminum Producing
Steel Producing

Metal Preparation and Pouring
Using Disinfectants or Biocides

Farming (Pesticides)
Sewer and Wastewater Treatment
Textiles (Printing, Dyeing, or Finishing)

Therapeutic Uses of Iron (III) Sulfate:
Seventy primary molar teeth, carious exposed, symptom free, without any sign of root resorption in children aged from 3 to 6 years (main age 4.3 yr) were treated with conventional pulpotomy procedures. 
Ferric sulfate 15.5% solution (applied for 15 second for 35 teeth) and formocresol solution (five minute procedure of Buckley's formula for next 35 teeth) have been used as pulpotomy agents. 

In both groups, pulp stumps were covered with zinc-oxide eugenol paste. 
Permanent restorations were stainless steel crowns. 

Clinical check up was every three-months and radiographic follow-up time was six and twenty months after treatment. 
Our results within this period revealed 100% clinical success rate in both groups. 
Radiographic success rate was in both groups 97.2%, while in 2.8% cases has shown internal root resorption.

The hemostatic efficacy, as well as the cardiovascular effects, of two hemostatic agents currently used during endodontic surgery was examined. 
The hemostatic agents used were epinephrine pellets (Racellet pellets) or 20% ferric sulfate (Viscostat). 

Patients were assigned to one of two experimental groups. 
Blood pressure and pulse rate were recorded pre- and postoperatively and at three additional times during the surgery (root-end resection, root-end preparation, and filling). 

The adequacy of hemostasis was rated by the surgical operator. 
Results indicated that there is no significant change in cardiovascular effects when using either of these hemostatic agents. 
Except in one case where ferric sulfate was the agent, both agents produced surgical hemostasis that allowed for a dry field for root-end filling.

Indication of Iron (III) Sulfate:
Ferric sulfate was first used in dermatology as part of the Monsel's solution. 
This solution is an antihemorrhagic agent used in skin and mucosal biopsies. 
The use of ferric sulfate in dermatology is under review as ferric sulfate is corrosive and injurious and Iron (III) Sulfate can cause degenerative changes that are not observed with other alternatives like collagen.

Ferric sulfate is also used as a coagulative and hemostatic agent. 
Iron (III) Sulfate is a mechanic hemostatic agent used directly on the damaged tissue.

In dentistry, ferric sulfate is used as a pulpotomy medicament to control pulpal bleeding, as an antibacterial agent and as a hemostatic reagent for restorative dentistry, for postextraction hemorrhage and for periradicular and endodontic surgery.

Pharmacodynamics of Iron (III) Sulfate:
The administration of ferric sulfate as a dermatologic agent has showed delayed reepithelialization and dyspigmentation. 
Some studies have reported the generation of inflammation in the sites of administration of ferric sulfate.

Mechanism action of Iron (III) Sulfate:
The main function of ferric sulfate is as a hemostatic agent in different medical practices. 
This hemostatic function is achieved when ferric sulfate is applied directly in the damaged tissue. 

Once applied, ferric sulfate forms ferric ion-protein complex which helps the sealing of the damaged vessels mechanically. 
The formation of agglutinated protein complexes produces the generation of occlusion in the capillary orifices.
The formation of the ferric protein complex is thought to be due to a chemical reaction between the acidic form of ferric sulfate and the blood proteins.

Protein binding of Iron (III) Sulfate:
Ferric sulfate presents very high protein binding properties, this property is thought to be due to Iron (III) Sulfate acidic profile.

Manufacturing and Production of Iron (III) Sulfate:

Ferric Sulfate is often generated commercially as a solution as opposed to being isolated as a solid. 
On a large scale, Iron (III) Sulfate is produced by treating sulfuric acid with a hot solution of ferrous sulfate, and an oxidizing agent such as chlorine, nitric acid, and hydrogen peroxide.

Methods of Manufacturing of Iron (III) Sulfate:
Prepared by treating iron(II) sulfate with boiling concentrated sulfuric acid, or by evaporating a mixture of iron(III) oxide and sulfuric acid. 
Iron(III) sulfate solutions are produced industrially by injecting chlorine gas into an iron(II) sulfate solution. 
The solution thus obtained contains a mixture of iron(III) sulfate and iron(III) chloride.

Production of Iron (III) Sulfate:
Ferric sulfate solutions are usually generated from iron wastes. 
The actual identity of the iron species is often vague, but many applications do not demand high purity materials. 
Iron (III) Sulfate is produced on a large scale by treating sulfuric acid, a hot solution of ferrous sulfate, and an oxidizing agent. 

Typical oxidizing agents include chlorine, nitric acid, and hydrogen peroxide.
2FeSO4 + H2SO4 + H2O2 → Fe2(SO4)3 + 2H2O

Natural occurrences of Iron (III) Sulfate:
Iron sulfates occur as a variety of rare (commercially unimportant) minerals. 
Mikasaite, a mixed iron-aluminium sulfate of chemical formula (Fe3+, Al3+)2(SO4)3 is the name of mineralogical form of iron(III) sulfate. 

This anhydrous form occurs very rarely and is connected with coal fires. 
The hydrates are more common, with coquimbite (nonahydrate) as probably the most often met among them. 

Paracoquimbite is the other, rarely encountered natural nonahydrate. 
Kornelite (heptahydrate) and quenstedtite (decahydrate) are rarely found. 

Lausenite (hexa- or pentahydrate) is a doubtful species. 
All the mentioned natural hydrates are unstable connected with the weathering (aerobic oxidation) of Fe-bearing primary minerals (mainly pyrite and marcasite).

Stability/Shelf Life of Iron (III) Sulfate:
Hydrolyzed slowly in aqueous solution.

Identification of Iron (III) Sulfate:

Analytic Laboratory Methods:
NIOSH Method: 268. 
Analyte: Sulfates. 
Matrix: Air. 
Procedure: Analysis by ion chromatography. 
Method Evaluation: Method was validated over the range of 0.1 to 10 mg/cu m using a 200 liter sample. 
Method detection limit: Approximately 0.5 ug/ml sulfate. 
Precision (CVT): 5%. 
Applicability: Under the conditions of sample size (200 l) the useful range is 0.25 to 5 mg/cu m. 
Interference: Insoluble sulfates need special care. 

Method 4500-Sulfate ion E. Turbidimetric Method for the determination of sulfate ion in water and wastewater. 
Sulfate ion is precipitated in an acetic acid medium with barium chloride so as to form barium sulfate crystals of uniform size. 

Light absorbance of barium sulfate suspension is measured by a photometer at 420 nm and the sulfate ion concentration is determined by comparison of the reading with a standard curve. 
This method is applicable in the range of 1 to 40 mg sulfate ion/l. 

The minimum detectable concentration is 1 mg sulfate/l. 
Interferences include suspended matter in large amounts, silica in excess of 500 mg/l and large quantities of organic material. 

With a turbidimeter, in a single laboratory with a sample having a mean of 7.45 mg sulfate ion/l, a standard deviation of 0.13 mg/l and a coefficient of variation of 1.7% were obtained. 
Two samples dosed with sulfate gave recoveries of 85 and 91%.

Method 4500-Sulfate ion F. Automated Methylthymol Blue Method for the determination of sulfate ions in water and wastewater. 
Barium sulfate is formed by the reaction of the sulfate ion with barium chloride at a low pH. 

At high pH, excess barium reacts with methylthymol blue to produce a blue chelate. 
The uncomplexed methylthymol blue is gray. 

The amount of gray uncomplexed methylthymol blue indicates the concentration of sulfate ion. 
To remove interferences from cations, an ion-exchange column is used. 

This method is applicable over a range of 10 to 300 mg sulfate ion/l. 
In a single laboratory a sample with an average concentration of about 28 mg sulfate/l had a standard deviation of 0.68 mg/l and a coefficient of variation of 2.4%. 
In two samples with added sulfate, recoveries were 91% and 100%.

EPA Method 9035. Colorimetric Automated Chloranilate Method applicalbe to ground water, drinking and surface waters, and domestic and industrial wastes containing 10 to 400 mg sulfate/liter. 
When solid barium chloranilate is added to a solution containing sulfate, barium sulfate is precipitated, releasing the highly colored acid chloranilate. 

Ions causing interference (calcium, aluminum, and iron) can be removed by passage through an ion exchange column. 
In a single laboratory, using surface water samples at concentrations of 38, 111, and 294 mg sulfate/l, the standard deviations were + or - 1.0, + or - 2.2, and + or - 0.8, respectively. 
In a single laboratory, using surface water samples at concentrations of 82 and 295 mg sulfate/l, recoveries were 99% and 102%, respectively. 

EPA Method 9038. Turbidimetric Method, applicable to ground water, drinking and surface waters, and domestic and industrial wastes. 
Sulfate ion is converted to a barium sulfate suspension under controlled conditions. 

The resulting turbidity is determined by a nephelometer, filter photometer, or spectrophotometer and compared with a curve prepared from standard sulfate solution. 
This method is suitable for all concentration ranges of sulfate; however, to obtain reliable readings, use a sample aliquot containing not more than 40 mg/l of sulfate. 

The minimum detectable limit is approximately 1 mg/l of sulfate. 
Silica in concentrations over 500 mg/l will interfere.

Sampling Procedures of Iron (III) Sulfate:
NIOSH Method 268. 
Analyte: Sulfates. 
Matrix: Air.
Procedure: Particulate sulfates and sulfites collected on filter, sulfur dioxide on treated filter. 
Flow Rate: 1.5 liters/min. 
Sample Size: 200 liters.

Handling and Storage of Iron (III) Sulfate:

Storage Conditions of Iron (III) Sulfate:
Keep well closed and protected from light.

Reactivity Profile of Iron (III) Sulfate:
Ferric Sulfate is acidic. 
Corrosive to copper, copper alloys, mild steel, and galvanized steel.

First Aid of Iron (III) Sulfate:
INHALATION: move to fresh air. 

INGESTION: give large amount of water; induce vomiting if large amounts have been swallowed. 

EYES: flush with water; get medical attention if irritation persists. 

SKIN: flush with water.

Fire Fighting of Iron (III) Sulfate:

Fire Fighting Procedures:
If material involved in fire: Extinguish fire using agent suitable for type of surrounding fire. 
(Material itself does not burn or burns with difficulty.)

Accidental Release Measures of Iron (III) Sulfate:

Cleanup Methods of Iron (III) Sulfate:
Environmental considerations, land spill: Dig a pit, pond, lagon, holding area to contain liquid or solid material. 
If time permits, pits, ponds, lagoons, soak holes, or holding areas should be sealed with an impermeable flexible membrane liner. 

Dike surface flow using soil, sand bags, foamed polyurethane, or foamed concrete. 
Absorb bulk liquid with fly ash, cement powder, or commercial sorbents.
Neutralize with agricultural lime, crushed limestone, or sodium bicarbonate.

Environmental considerations, water spill: Neutralize with agricultural lime, crushed limestone, or sodium bicarbonate. 
Adjust pH to neutral (pH= 7). 
Use mechanical dredges or lifts to remove immobilized masses of pollutants and precipitates.

Disposal Methods of Iron (III) Sulfate:
The most favorable course of action is to use an alternative chemical product with less inherent propensity for occupational exposure or environmental contamination. 
Recycle any unused portion of the material for Iron (III) Sulfate approved use or return Iron (III) Sulfate to the manufacturer or supplier. 

Ultimate disposal of the chemical must consider: the material's impact on air quality.
Potential migration in soil or water.

Effects on animal, aquatic, and plant life.
And conformance with environmental and public health regulations.

Preventive Measures of Iron (III) Sulfate:
The scientific literature for the use of contact lenses in industry is conflicting. 
The benefit or detrimental effects of wearing contact lenses depend not only upon the substance, but also on factors including the form of the substance, characteristics and duration of the exposure, the uses of other eye protection equipment, and the hygiene of the lenses. 

However, there may be individual substances whose irritating or corrosive properties are such that the wearing of contact lenses would be harmful to the eye. 
In those specific cases, contact lenses should not be worn. 
In any event, the usual eye protection equipment should be worn even when contact lenses are in place.

If material not involved in fire: Keep material out of water sources and sewers. 
Build dikes to contain flow as necessary.

Personnel protection: Keep upwind.
Avoid breathing vapors or dusts. 
Wash away any material which may have contacted the body with copious amounts of water or soap and water.

All iron preparations should be kept in child-proof bottles.

Identifiers of Iron (III) Sulfate:
CAS Number: 10028-22-5
ChEBI: CHEBI:53438
ChemSpider: 23211
ECHA InfoCard: 100.030.054
PubChem CID: 24826
RTECS number: NO8505000
UNII: 4YKQ1X5E5Y
CompTox Dashboard (EPA): DTXSID5029712
InChI:
InChI=1S/2Fe.3H2O4S/c;;3*1-5(2,3)4/h;;3*(H2,1,2,3,4)/q2*+3;;;/p-6
Key: RUTXIHLAWFEWGM-UHFFFAOYSA-H check
InChI=1/2Fe.3H2O4S/c;;3*1-5(2,3)4/h;;3*(H2,1,2,3,4)/q2*+3;;;/p-6
Key: RUTXIHLAWFEWGM-CYFPFDDLAR
SMILES: [Fe+3].[Fe+3].[O-]S(=O)(=O)[O-].[O-]S([O-])(=O)=O.[O-]S([O-])(=O)=O

Chemical Identifiers of Iron (III) Sulfate:
Linear Formula: Fe2(SO4)3
MDL Number: MFCD00011007
EC No.: 233-072-9
Pubchem CID: 24826
IUPAC Name: 
iron(3+)
trisulfate
SMILES: [O-]S(=O)(=O)[O-] .[O-]S(=O)(=O)[O-] .[O-]S(=O)(=O)[O-] .[Fe+3].[Fe+3]
InchI Identifier: InChI=1S/2Fe.3H2O4S/c;;3*1-5(2,3)4/h;;3*(H2,1,2,3,4)/q2*+3;;;/p-6
InchI Key: RUTXIHLAWFEWGM-UHFFFAOYSA-H

Properties of Iron (III) Sulfate:
Chemical formula: Fe2(SO4)3
Molar mass: 
399.88 g/mol (anhydrous)
489.96 g/mol (pentahydrate)
562.00 g/mol (nonahydrate)
Appearance: grayish-white crystals
Density: 
3.097 g/cm3 (anhydrous)
1.898 g/cm3 (pentahydrate)
Melting point: 
480 °C (896 °F; 753 K) (anhydrous)
175 °C (347 °F) (nonahydrate)
Solubility in water: 256g/L (monohydrate, 293K)
Solubility: 
sparingly soluble in alcohol negligible in acetone, ethyl acetate
insoluble in sulfuric acid, ammonia
Refractive index (nD): 
1.814 (anhydrous)
1.552 (nonahydrate)

Molecular Weight: 399.9
Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 12
Rotatable Bond Count: 0
Exact Mass: 399.725060
Monoisotopic Mass: 399.725060
Topological Polar Surface Area: 266 Ų
Heavy Atom Count: 17
Complexity: 62.2    
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 5
Compound Is Canonicalized: Yes

Quality Level: 200
Assay: 97%
Form: powder
Reaction suitability:
reagent type: catalyst
core: iron
SMILES string:[Fe+3].[Fe+3].[O-]S([O-])(=O)=O.[O-]S([O-])(=O)=O.[O-]S([O-])(=O)=O
InChI: 1S/2Fe.3H2O4S/c;;3*1-5(2,3)4/h;;3*(H2,1,2,3,4)/q2*+3;;;/p-6
InChI key: RUTXIHLAWFEWGM-UHFFFAOYSA-H

Alternate Chemical Names of Iron (III) Sulfate:
AMERSEP 5320
DIIRON TRISULFATE
DIIRON(3+) SULFATE
FERRIC SULFATE
FERRIC SULPHATE
IRON (III) SULFATE
IRON PERSULFATE
IRON SESQUISULFATE
IRON SULFATE (2:3)
IRON SULFATE (FE2(SO4)3)
IRON(3+) SULFATE
IRON(III) SULFATE

Related compounds of Iron (III) Sulfate:
Iron(II) sulfate

Other anions of Iron (III) Sulfate:    
Iron(III) chloride
Iron(III) nitrate

Names of Iron (III) Sulfate:

IUPAC name of Iron (III) Sulfate:
Iron(III) sulfate

Other names of Iron (III) Sulfate:
Ferric sulfate

Synonyms of Iron (III) Sulfate:
FERRIC SULFATE
10028-22-5
Iron(III) sulfate
Iron persulfate
Iron tersulfate
Iron(3+) sulfate
Diiron tris(sulphate)
Diiron trisulfate
Ferric persulfate
Ferric tersulfate
Iron sesquisulfate
Ferric sesquisulfate
iron(3+);trisulfate
UNII-4YKQ1X5E5Y
MFCD00011007
4YKQ1X5E5Y
Coquimbite mineral
Iron sulfate (2:3)
Iron sulfate (Fe2(SO4)3)
CCRIS 7885
Iron(3+) sulfate, (2:3)
HSDB 6311
EINECS 233-072-9
Sulfuric acid, iron(3+) salt
Iron-S-hydrate
iron(III)sulphate
Ferric sulfate (USP)
Sulfuric acid,iron salt
iron(III) sulfate(VI)
Diiron trissulfate hydrate
Polyferric sulfate(SPFS)
Diiron trissulphate hydrate
EC 233-072-9
Iron (lll) sulfate hydrate
Iron(III) sulphate hydrate
2Fe.3SO4
DTXSID5029712
CHEBI:53438
5184AF
Iron(III) sulfate (Fe2(SO4)3)
FERRIC SULFATE HYDRATE 500GM
AKOS015903761
FT-0627289
D08922
Q409021
Iron(III) sulfate 
10028-22-5
diferric trisulfate
Diiron tris(sulphate)
DIIRON TRISULFATE
Eisen(3+)sulfat (2:3)
Ferric sulfate
Ferric Sulphate
iron (III) sulfate
Iron(3+) sulfate (2:3)
Iron(III) sulphate
Sulfate de fer(3+) (3:2)
1310-45-8
13761-89-2
15244-10-7
233-072-9
35139-28-7
Coquimbite mineral
FERRIC PERSULFATE
Ferric sesquisulfate
Ferric Sulfate, Hydrate
Ferric tersulfate
ferricsulfate
IRON PERSULFATE
Iron sesquisulfate
IRON SULFATE (2:3)
Iron tersulfate
iron(+3) cation trisulfate
IRON(3+) SULFATE
Iron(3+) sulfate, (2:3)
iron(III) sulfate(VI)
MFCD00011007
MFCD00149714 
Sulfuric acid, iron salt
Sulfuric acid, iron(3+) salt
SULFURIC ACID, IRON(3+) SALT (3:2)
Sulfuric acid,iron salt