Ferric Sulfate

3.1 at 68 °F (USCG, 1999) - Denser than water; will sink

3.097 at 18 °C

3.1 @25 °C

Grayish-white powder, or rhombic or rhombohedral crystals

Yellow crystals

Soluble at room temperature

Slowly sol in water; rapidly sol in the presence of a trace of ferrous sulfate; sparingly sol in alc; practically insol in acetone, ethyl acetate.

Insol in sulfuric acid, ammonia

The Anhydrous form decomposes (480ºC)

480 °C (decomp)

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 its spread to the environment. It is used for water purification, and as a soil conditioner.

Wet Solid; Liquid; Other Solid; Large Crystals; Liquid; Liquid

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

MW 562.00; rhombic crystals; deliquescent; index of refraction 1.552, 1.553; density 2.1; MP 175 °C (loses 7H2O); solubility 440 g/100 ml in cold water; decomp in hot water; sol in abs alc. /Iron(III) sulfate, enneahydrate/

Commercial product usually contains about 20% water and is yellowish in color; very hygroscopic; hydrolyzed slowly in aqueous solution

Yellow brown /Iron(III) sulfate, enneahydrate/

Density 2.0-2.1; melting point, decomposes at 480 °C; very soluble in water /Nonahydrate/

This chemical does not meet GHS hazard criteria for 0.4% (2 of 446) of reports.

Danger

H290 (40.4%): May be corrosive to metals [Warning Corrosive to Metals]；H302 (90.1%): Harmful if swallowed [Warning Acute toxicity, oral]；H315 (87.7%): Causes skin irritation [Warning Skin corrosion/irritation]；H317 (11.4%): May cause an allergic skin reaction [Warning Sensitization, Skin]；H318 (80.7%): Causes serious eye damage [Danger Serious eye damage/eye irritation]；H319 (18.8%): Causes serious eye irritation [Warning Serious eye damage/eye irritation]；H335 (20.4%): May cause respiratory irritation [Warning Specific target organ toxicity, single exposure; Respiratory tract irritation]

P234, P261, P264, P264+P265, P270, P271, P272, P280, P301+P317, P302+P352, P304+P340, P305+P351+P338, P305+P354+P338, P317, P319, P321, P330, P332+P317, P333+P317, P337+P317, P362+P364, P390, P403+P233, P405, P406, and P501 (click each P-code to see the statement)

Aggregated GHS information provided per 446 reports by companies from 19 notifications to the ECHA C&L Inventory. Each notification may be associated with multiple companies.；Reported as not meeting GHS hazard criteria per 2 of 446 reports by companies.；There are 18 notifications provided by 444 of 446 reports by companies with hazard statement code(s).；Information may vary between notifications depending on impurities, additives, and other factors. The percentage value in parenthesis indicates the notified classification ratio from companies that provide hazard codes. Only hazard codes with percentage values above 10% are shown. For more detailed information, please visit ECHA C&L website.

Chemical: Sulfuric acid, iron(3+) salt (3:2)

Hazard Traits - Respiratory Toxicity；Authoritative List - OEHHA RELs；Report - if used as a fragrance or flavor ingredient

Sulfuric acid, iron(3+) salt (3:2) is listed on the EPA's Chemical Data Reporting (CDR) system. Manufacturers and importers of Sulfuric acid, iron(3+) salt (3:2) are required to report information about their production and use of this chemical to the EPA under the Toxic Substances Control Act (TSCA). (40 eCFR Part 711)

Status: Active Update: 17-04-2020 https://echa.europa.eu/registration-dossier/-/registered-dossier/15372

Sulfuric acid, iron (III) salt: Does not have an individual approval but may be used under an appropriate group standard

The New Jersey Worker and Community Right to Know Act requires public and private employers to provide information about hazardous substances at their workplaces. (N.J.S.A. 34:5A-1 et. seq.)

Substance added directly to human food affirmed as generally recognized as safe (GRAS).

Trace minerals added to animal feeds. These substances added to animal feeds as nutritional dietary supplements are generally recognized as safe when added at levels consistent with good feeding practice. All substances listed may be in anhydrous or hydrated form. Iron sulfate is included on this list. /Iron Sulfate/

Residues of ferric sulfate are exempted from the requirement of a tolerance when used as a solid diluent or carrier in accordance with good agricultural practices as inert (or occasionally active) ingredients in pesticide formulations applied to growing crops or to raw agricultural commodities after harvest.

Environmental considerations, land spill: Dig a pit, pond, lagon, holding area to contain liquid or solid material. /SRP: 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.

SRP: 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 its approved use or return it 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.

SRP: 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. /Iron preparations/

Residues of ferric sulfate are exempted from the requirement of a tolerance when used as a solid diluent or carrier in accordance with good agricultural practices as inert (or occasionally active) ingredients in pesticide formulations applied to growing crops or to raw agricultural commodities after harvest.

1.0 [mg/m3], as Fe (soluble iron salts)

Time Weighted Avg (TWA) 1 mg/cu m. /Iron salts, soluble, as Fe/

Excursion Limit Recommendation: Excursions in worker exposure levels may exceed 3 times the TLV-TWA for no more than a total of 30 minutes during a work day, and under no circumstances should they exceed 5 times the TLV-TWA, provided that the TLV-TWA is not exceeded. /Iron salts, soluble, as Fe/

0.55 [mg/m3]

6.1 [mg/m3]

36 [mg/m3]

Dust mask; goggles or face shield; protective gloves (USCG, 1999)

/NIOSH certified respirator/; goggles or face shield.

Australia, Belgium, Finland, Italy, Netherlands, & Switzerland: 1 mg/cu m. /Iron salts/

Australia (1978); Belgium (1978); Finland (1975); Italy (1978); Netherlands (1978); and Switzerland (1978): 1 mg/cu m. /From table/ /Ferric salts, as Fe/

...A brief exposure (1 hr) of 51Cr-radiolabeled breast cancer cells (BT-20) but not colon cancer cells (Caco-2) to hemin (10 uM) or FeSO4 (10 uM) significantly enhances cytotoxicity mediated by 0.5 mM hydrogen peroxide (H2O2). Associated with Caco-2 resistance, these cells were found to be enriched in the endogenous iron chelator, ferritin. If cellular ferritin is even further increased through 1 hr incubation (24 hr prior to H2O2 exposure) of both cell types with hemin, FeSO4, or exogenous spleen apoferritin itself (24 hr), marked resistance to H2O2-mediated cytotoxicity is manifest. Under several conditions, the sensitivity of tumor cells to oxidant-mediated lysis is inversely proportional to their ferritin content. Pretreatment of BT-20 and Caco-2 cells with hemin or FeSO4 rapidly increases H-ferritin mRNA but only slightly increases L-ferritin mRNA; nevertheless, large increases in overall ferritin content of iron-exposed cells result. Data analogous to those with H2O2-mediated cytotoxicity were obtained in studies of bleomycin-engendered DNA strand breakage and cell damage, i.e., brief treatment of BT-20 cells with both hemin or FeSO4 significantly increases their sensitivity to bleomycin (100 ug/mL), whereas treatment followed by 24 hr incubation with media alone significantly protects against bleomycin toxicity.

LD50 Colinus virginianus (Northern bobwhite) oral via capsule >2250 mg/kg, 14 day exposure

LC50 Gambusia affinis (Western mosquitofish) 37.2 mg/L/24, 48, 96 hr; static

LC50 Salmo trutta (Brown trout) 28 mg total Fe/L (0.05 mg soluble Fe/L)/96 hr /Conditions of bioassay not specified in source examined/ /Commercial iron (III) sulphate liquor/

LC50 Salmo trutta (Brown trout) 47 mg total Fe/L (0.24 mg soluble Fe/L)/96 hr /Conditions of bioassay not specified in source examined/ /Analar grade iron (III) sulphate/

/AQUATIC SPECIES/ The 96-hr LC50 on brown trout Salmo trutta of a commercial iron (III) sulphate liquor, used for treating reservoirs to reduce algal growth, was 28 mg total Fe/L (0.05 mg soluble Fe/L). The 96-hr LC50 for analar grade iron (III) sulphate was 47 mg total Fe/L (0.24 mg soluble Fe/L). Lethal and sublethal exposure to both grades of iron resulted in accumulation on the gill, which appears to be the main target for iron toxicity /in brown trout (Salmo trutta)/. Greater iron accumulation occurred during exposure to commercial iron sulfate liquor. Physical clogging of gills and gill damage was seen during lethal and sublethal exposure to iron. Gill tissue analysis showed no evidence of iron uptake into gill tissues during lethal or sublethal exposure to iron. Iron did not accumulate in plasma of fish exposed to iron compared to controls. Respiratory disruption due to physical clogging of the gills is suggested as a possible mechanism for iron toxicity.

/AQUATIC SPECIES/ ...The acute and chronic effects upon Daphnia longispina, the dominant member of the zooplankton. Laboratory tests established that, although dissolved iron had no measurable effect, the presence of particulate iron caused mortalities in acute tests (48 hours) and reduced number of broods per female and numbers of young hatching in chronic tests (21 days). At 11.48 mg Fe/L, 50% mortalities occurred in the population, /while/ 4.49 mg Fe/L caused reductions in reproduction and increased mortality rates over 21 day tests. In inert china clay, similar results were observed, suggesting that it was the particulate nature of the ferric sulfate that caused the effects, rather than any toxic properties. A safe level of 1.69 mg Fe/L was calculated. The area of the filter of the third thoracic limb of the daphnids, from both the laboratory cultures and the south arm of Rutland Water (which received ferric-dosed inlet water) increased in size in the presence of ferric sulfate and china clay in chronic tests. This is a response to low food concentrations. Abnormal feeding behavior was also observed in ferric sulfate. Thoracic beat rate, decreased in ferric sulfate but was unaffected in china clay. This suggested that the feeding rate depression was a response to the chemical nature of the ferric sulfate, rather than its particulate nature. The number of times that particles were rejected from the food groove increased in both ferric sulfate and china clay, in response to large clumps of these substances collecting there.

/HUMAN EXPOSURE STUDIES/ Twenty normal and 18 asthmatic human volunteers were exposed to ferric sulfate aerosol at a nominal concentration of 75 ug/cu m (equivalent to 20 ug iron/cu m). The concentration and particle size distribution (2 micron mass median aerodynamic diameter; geometric standard deviation of 3) were selected to simulate worst case ambient conditions. Ferric sulfate was chosen for study because it is toxic, it is a respiratory system irritant, and increased use of coal and high sulfur fuel oils will lead to increased concentrations of iron and sulfate in ambient air. A double blind protocol was followed in which each subject was exposed on two days, separated by about a three week period. The subjects were exposed to clean air (sham) on one day and to ferric sulfate aerosol on the other (exposure); the order of exposure was selected randomly. Neither the subjects nor the staff performing the clinical testing were informed as to the nature of the atmosphere on any given day. Pulmonary function tests were performed immediately before (pre) and after (post) each 2 hr sham or exposure period; this protocol included intermittent exercise. Pre and postexposure symptom score interviews were also administered. On the average, the two groups of subjects did not exhibit significant pre to postchanges in total respiratory system resistance, forced expiratory flow/volume performance, and single breath nitrogen washout parameters. None of the subjects reported more than slight changes in symptoms during exposure. Five individuals showed small but significant decremental trends in pulmonary function; however, nine subjects tended to improve after exposure.

/LABORATORY ANIMALS: Acute Exposure/ .../iron-sulfate/ or vehicle (dimethylsulfoxide or aqueous ethanol) alone was applied to the dorsum of each ear of female BALB/c-mice for 3 consecutive days; in some animals, the dorsal surface of the ear was gently abraded by needle just prior to metal salt application. Mice were sacrificed 4 days after the initial application for preparation and analysis of /lymph node cells/ (LNCs). Results were expressed as the stimulation indices value resulting in an increase of lymphocyte proliferation in draining lymph nodes relative to vehicle treated groups. While nickel, cobalt, chromium, and copper salts increased LNC proliferation, zinc, manganese, and iron salts did not. LNC proliferation tended to increase with increased concentration of metal salt.

/LABORATORY ANIMALS: Subchronic or Prechronic Exposure/ A study was performed to provide data on the disposition, accumulation and toxicity of sodium iron EDTA in comparison with iron (II) sulfate in rats on administration via the diet for 31 and 61 days. ...Iron is accumulated from the diet in liver, spleen and kidneys in a dose-dependent manner, and iron derived from FeEDTA is taken up and/or accumulated less efficiently in liver and spleen than iron from FeSO(4). Moreover, feeding iron up to 11.5 and 11.2 mg/kg bw/day, derived from FeSO(4) and FeEDTA, respectively, did not result in tissue iron excess nor in any other toxicologically significant effects.

/LABORATORY ANIMALS: Subchronic or Prechronic Exposure/ ...Standardized osseous defects were created bilaterally in the naturally edentulous zone in rabbit mandibles. The control site was sutured immediately after clot formation in the defect. The contralateral experimental site received ferric sulfate application until complete hemostasis was achieved. The defect was filled with ferric sulfate solution to maximize any effect on healing and then closed with sutures. The experimental and control specimens were examined histologically after 18 and 46 days and scored for healing. Statistical analysis by Wilcoxon signed rank test showed significant adverse effects on osseous healing when ferric sulfate solution was left in situ.

...There is concern that the individual with metabolic defects that impair the ability to regulate iron absorption will be at risk from excessive exposure to iron, primarily as a result of acceleration of accumulation of iron in the body and an earlier onset of clinical symptoms of the disease. /Iron salts/

Basic treatment: Establish a patent airway. Suction if necessary. Watch for signs of respiratory insufficiency and assist ventilations if necessary. Administer oxygen by nonrebreather mask at 10 to 15 L/min. Monitor for shock and treat if necessary ... . For eye contamination, flush eyes immediately with water. Irrigate each eye continuously with normal saline during transport ... . Do not use emetics. For ingestion, rinse mouth and administer 5 ml/kg up to 200 ml of water for dilution if the patient can swallow, has a strong gag reflex, and does not drool. /Iron and related compounds/

Advanced treatment: Consider orotracheal or nasotracheal intubation for airway control in the patient who is unconscious. Monitor cardiac rhythm and treat arrhythmias if necessary ... . Start an IV with lactated Ringer's /SRP: "To keep open", minimal flow rate/. Watch for signs of fluid overload. For hypotension with signs of hypovolemia, administer fluid cautiously. Watch for signs of fluid overload ... . Use proparacaine hydrochloride to assist eye irrigation ... . /Iron and related compounds/

Maintain an open airway and assist ventilation if necessary. Treat shock caused by hemorrhagic gastrointestinitis aggressively with intravenous crystalloid fluids, and replace blood if needed. Patients are often markedly hypovolemic owing to gastrointestinal losses and third spacing of fluids into the intestinal wall and interstitial space. Treat coma, seizures, and metabolic acidosis if they occur. For seriously intoxicated victims (eg, shock, severe acidosis, and/or serum iron > 500-600 mcg/dL) administer deferoxamine. Monitor the urine for the urine for the characteristic orange or pink deferoxamine-iron complex. Therapy may be stopped when the urine returns to normal or when the serum iron level decreases to the normal range. Prolonged deferoxamine has been associated with adult respiratory distress syndrome and Yersinia sepsis.

Activated charcoal is not effective. Ipecac is not recommended, because it can aggravate iron-induced gastrointestinal irritation and interfere with whole bowel irrigation. Consider gastric lavage if product was a liquid formulation or tablets were chewed. Do-not use phosphate-containing solutions for lavage; these may result in life-threatening hypernatremia, hyperphosphatemia, and hypocalcemia. Bicarbonate and deferoxamine lavage are of doubtful efficacy. Deferoxamine lavage is not effective and may enhance iron absorption. Whole-bowel irrigation is very effective for ingested tablets and may be considered first-line treatment, especially if large numbers of tablets are visible on plain abdominal x-ray. Massive ingestions may lead to concretions or bezoars. Repeated or prolonged whole-bowel irrigation may remove tablets. Endoscopy or surgical gastrotomy is rarely required.

Hemodialysis and hemoperfusion are not effective for removing iron but may be necessary to remove iron-deferoxamine complex in patients with renal failure. Exchange transfusion is occasionally used for massive pediatric ingestions but is of questionable efficacy.

Chemical: Sulfuric acid, iron(3+) salt (3:2)

Hazard Traits - Respiratory Toxicity；Authoritative List - OEHHA RELs；Report - if used as a fragrance or flavor ingredient

Sulfuric acid, iron(3+) salt (3:2) is listed on the EPA's Chemical Data Reporting (CDR) system. Manufacturers and importers of Sulfuric acid, iron(3+) salt (3:2) are required to report information about their production and use of this chemical to the EPA under the Toxic Substances Control Act (TSCA). (40 eCFR Part 711)

Status: Active Update: 17-04-2020 https://echa.europa.eu/registration-dossier/-/registered-dossier/15372

Sulfuric acid, iron (III) salt: Does not have an individual approval but may be used under an appropriate group standard

The New Jersey Worker and Community Right to Know Act requires public and private employers to provide information about hazardous substances at their workplaces. (N.J.S.A. 34:5A-1 et. seq.)

Substance added directly to human food affirmed as generally recognized as safe (GRAS).

Trace minerals added to animal feeds. These substances added to animal feeds as nutritional dietary supplements are generally recognized as safe when added at levels consistent with good feeding practice. All substances listed may be in anhydrous or hydrated form. Iron sulfate is included on this list. /Iron Sulfate/

Residues of ferric sulfate are exempted from the requirement of a tolerance when used as a solid diluent or carrier in accordance with good agricultural practices as inert (or occasionally active) ingredients in pesticide formulations applied to growing crops or to raw agricultural commodities after harvest.

Persons in charge of vessels or facilities are required to notify the National Response Center (NRC) immediately, when there is a release of this designated hazardous substance, in an amount equal to or greater than its reportable quantity of 1000 lb or 454 kg. The toll free number of the NRC is (800) 424-8802; In the Washington D.C. metropolitan area (202) 426-2675. The rule for determining when notification is required is stated in 40 CFR 302.4 (section IV. D.3.b).

Ferric sulfate is designated as a hazardous substance under section 311(b)(2)(A) of the Federal Water Pollution Control Act and further regulated by the Clean Water Act Amendments of 1977 and 1978. These regulations apply to discharges of this substance. This designation includes any isomers and hydrates, as well as any solutions and mixtures containing this substance.

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.

FERRIC SULFATE

Phosphate Binder [EPC]; Iron [CS]; Parenteral Iron Replacement [EPC]; Phosphate Chelating Activity [MoA]

Pharmacokinetic studies related to the absorption of ferric sulfate have not been performed.

Pharmacokinetic studies related to the elimination of ferric sulfate have not been performed.

Pharmacokinetic studies related to the volume of distribution of ferric sulfate have not been performed.

Pharmacokinetic studies related to the clearance of ferric sulfate have not been performed.

The bioavailability of ferrous and ferric iron following cecal infusion was compared by assessing the hemoglobin regeneration method in ileally fistulated anemic rats. Rats were fed an iron-deficient diet (8 mg Fe/kg diet) for 14 days after recovery from surgery. The anemic rats were then divided into three groups of 11 rats. Group 1 (control) was fed an iron-adequate diet (45 mg Fe/kg diet) and infused with NaCl solution (150 mM). Group 2 and 3 were fed an iron-deficient diet and infused with ferrous sulfate [Fe(II)] suspension or ferric sulfate [Fe(III)] solution (800 ppm as Fe, pH 6.8) to provide the same amount of iron as that consumed one day before by the control group. NaCl, Fe(II) and Fe(III) were infused through the fistula as two times (1000 hr and 1800 hr) for 14 days. The volume of NaCl infused was about equal to the volume of Fe(II) suspension and Fe(III) solution infused. Hemoglobin regeneration efficiency, hematocrit, plasma iron concentration, transferrin saturation, total iron-binding capacity, iron contents in organs (liver, spleen and kidney), body weight gain and food intake were almost the same among groups.

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; [HSDB]

Aluminum Producing [Category: Industry]；Steel Producing [Category: Industry]；Metal Preparation and Pouring [Category: Foundry]；Using Disinfectants or Biocides [Category: Clean]；Farming (Pesticides) [Category: Industry]；Sewer and Wastewater Treatment [Category: Industry]；Textiles (Printing, Dyeing, or Finishing) [Category: Industry]

For ferric sulfate (USEPA/OPP Pesticide Code: 034902) ACTIVE products with label matches. /SRP: Registered for use in the U.S. but approved pesticide uses may change periodically and so federal, state and local authorities must be consulted for currently approved uses./

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.

Fertilizer /Iron(III) sulfate, enneahydrate/

Plating agent；Deodorizer；Processing aids not otherwise specified；Soil amendments (fertilizers)；Not Known or Reasonably Ascertainable；Cleaning agent；Softener and conditioner；Etching agent；Adhesion/cohesion promoter；Chelating agent；Flocculating agent；Solids separation (precipitating) agent, not otherwise specified；Intermediate

... 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.

By adding sulfuric acid to ferric hydroxide.

Grades: Technical, CP, partly hydrated

Fertilizer grade material contains about 21.2% iron, or 30.3% iron trioxide /Iron(III) sulfate, enneahydrate/

/Available as/ hydrated reagent grades; liquid and dry grades

Fabricated Metal Product Manufacturing；Petroleum Refineries；Not Known or Reasonably Ascertainable；All Other Chemical Product and Preparation Manufacturing；Wood Product Manufacturing；Food, beverage, and tobacco product manufacturing；Paper Manufacturing；Machinery Manufacturing；Utilities；Mining (except Oil and Gas) and support activities；All Other Basic Inorganic Chemical Manufacturing；Transportation Equipment Manufacturing；Electrical Equipment, Appliance, and Component Manufacturing；Computer and Electronic Product Manufacturing；Wholesale and Retail Trade；Agriculture, Forestry, Fishing and Hunting

Sulfuric acid, iron(3+) salt (3:2): ACTIVE

A quickly available source of iron. /Iron(III) sulfate, enneahydrate/

Coquimbite /Iron(III) sulfate, enneahydrate/