Pharmacological properties of the drug Iron sulfate
Ferrous iron, which is part of the salt, compensates for the deficiency of this microelement in the body (in particular in iron deficiency anemia), stimulates erythropoiesis, and takes part in metabolic processes. Iron ions are components of hemoglobin, myoglobin, and many enzymes. Iron deficiency in the body occurs when there is a lack of this element in food, when absorption in the digestive tract is impaired (diarrhea, large-scale operations associated with resection of the stomach, intestines), with an increased need for iron (pregnancy, active growth), with blood loss (hypermenorrhea , hemorrhagic complications during surgical interventions). When carrying out a course of treatment of iron deficiency anemia, there is a gradual regression of clinical signs of anemia (general weakness, fatigue, dizziness, tachycardia, soreness and dry skin) and laboratory test indicators. 325 mg of iron sulfate corresponds to 0.105 g of elemental iron.
Is it possible to get an overdose?
Ferrous sulfate is safe if you take it as directed by a qualified healthcare professional. However, this compound—and any other iron supplement—can be toxic in large quantities, especially to children (, ).
Some symptoms that can result from taking too much ferrous sulfate are coma, convulsions, organ failure and even death ().
Therefore, it is extremely important to never take more ferrous sulfate than recommended by your doctor.
Summary:
Ferrous sulfate supplements can be toxic and even fatal in large quantities. Never take more than the dosage recommended by your doctor, and always keep supplements out of the reach of children.
Spraying trees
Experienced summer residents consider this manipulation an important procedure. They note that before spraying garden crops, it is important to properly prepare a solution of iron sulfate, avoiding too strong a concentration.
For prevention and control of harmful insects, moss and various types of lichen, a 5% composition is prepared (500 g of the substance is dissolved in a bucket of water). Spraying is carried out twice a year, in early spring and autumn after harvesting. For the treatment of shrub and stone fruit crops, the same schedule is followed, however, the concentration in this case should be lower (300 g of substance per 10 liters of water).
For chemists and technologists, iron sulfate is one of the many chemical compounds that can be obtained artificially. For a person far from this science, iron sulfate is a remedy that helps solve pressing everyday issues in the garden, construction, and medicine.
The article discusses the production and use of ferrous sulfate in industry and for people's livelihoods at home, and describes its use for the treatment of certain diseases in children and adults. A detailed description of the use of this substance in gardening is also given.
Usage
- As a reagent for hydrometallurgical processing of copper ores.
- As a coagulant in the treatment of wastewater, municipal and industrial wastewater.
- As a mordant for dyeing fabrics.
- When tanning leather.
- For pickling of stainless austenitic steels, gold and aluminum alloys.
- As a flotation regulator to reduce the buoyancy of ores.
- In medicine it is used as an astringent and hemostatic agent.
- In the chemical industry as an oxidizer and catalyst.
Application in horticulture
This is one of the most important branches of agriculture, therefore iron sulfate is used here quite widely. The main methods of application are sanitary treatment of premises, preventive impregnation of wood against house fungus, whitewashing of young plantings in the spring.
Iron sulfate is best suited for protecting flowers and garden crops from pests. To do this, the plants are sprayed with a ready-made iron-based solution, which, in addition, begin to bloom more luxuriantly. That is, the substance also serves as a nutritious bait. It is worth knowing that lime cannot be added to it; only copper sulfate is allowed.
To achieve the best result, it is necessary to add mineral foliar fertilizers to the soil in the form of an aqueous solution (5 g per bucket of water). Such fertilizing will have a beneficial effect on the yield of, for example, strawberries and currants. It is equally effective to use it in combination with compost. The dosage in this case should be 100 g per bucket of organic matter. By feeding garden crops in this way, you can reap a rich harvest in the fall, which will be significantly larger in volume than what was grown without fertilizer.
Links[edit]
- ^ abcdef "Mineral data of Siderotile". Retrieved August 3, 2014.
- ^ abcdef "Ferrohexahydrite Mineral Data". Retrieved August 3, 2014.
- ^ abcdefgh Leede, David R., ed. (2009). CRC Handbook of Chemistry and Physics
(90th ed.). Boca Raton, FL: CRC Press. ISBN 978-1-4200-9084-0. - ^ ab Seidell, Atherton; Linke, William F. (1919). Solubility of inorganic and organic compounds (2nd ed.). New York: D. Van Nostrand Company. paragraph 343.
- ^ a b Anatolyevich, Kiper Ruslan. "iron(II) sulfate". Retrieved August 3, 2014.
- ^ abcd Sigma-Aldrich Co. , Iron(II) sulfate heptahydrate. Retrieved August 3, 2014.
- ^ abcde Ralph, Jolyon; Chautitle, Ida. "Somolnokite". mindat.org. Retrieved August 3, 2014.
- ^ abcde "Mineral data of rosenite". Retrieved August 3, 2014.
- ^ abcde "Melanterite Mineral Data". Retrieved August 3, 2014.
- ^ab "Safety Data Sheet for Ferrous Sulfate Heptahydrate". Fair Lawn, New Jersey: Fisher Scientific, Inc. Retrieved August 3, 2014.
- ^ abcd Weil, Matthias (2007). "High temperature β-modification of iron(II) sulfate". Acta Crystallographica Section
E.
International Union of Crystallography. 63
(12):i192. DOI: 10.1107/S160053680705475X. Retrieved August 3, 2014. - ^ abcd Anatolyevich, Kiper Ruslan. "iron(II) sulfate heptahydrate". Retrieved August 3, 2014.
- NIOSH Pocket Guide to Chemical Hazards. "#0346" . National Institute of Occupational Safety and Health (NIOSH).
- beta-static.fishersci.com/content/dam/fishersci/en_US/documents/programs/education/regulatory-documents/sds/chemicals/chemicals-f/S25325A.pdf
- Brown, Leslie (1993). The New Shorter Oxford English Dictionary on Historical Principles. Oxford [English]: Clarendon. ISBN 0-19-861271-0.
- World Health Organization (2019). World Health Organization Model List of Essential Medicines: 2019 Top Twenty List
. Geneva: World Health Organization. HDL: 10665/325771. WHO/MVP/EMP/IAU/2022.06. License: CC BY-NC-SA 3.0 IGO. - "Top 300 2022". ClinCalc
. Retrieved February 18, 2022. - "Ferrous Sulfate - Drug Use Statistics". ClinCalc
. Retrieved February 18, 2022. - British Journal of Archaeology. https://www.archaeologyuk.org/ba/ba66/feat2.shtml (archive)
- Torczyner, Lachish Letters
, pp. 188–95 - ↑
Hyatt,
The Interpreter's Bible
, 1951, volume V, page 1067 - How to paint concrete with ferrous sulfate
- “Why use ferrous sulfate on lawns?” . Retrieved April 14, 2022.
- "Acidic or Alkaline Soil: Changing pH - Sunset Magazine". www.sunset.com
. Retrieved April 14, 2022. - Koenig, Rich and Kuhns, Mike: Control of iron chlorosis in ornamental crop plants
. (University of Utah, Salt Lake City, August 1996) p. - ^ ab Handrek, Kevin (2002). Gardening Below: A Guide to Healthier Soils and Plants
(2nd ed.). Collingwood, Victoria: CSIRO Publishing. pp. 146–47. ISBN 0-643-06677-2. - Brothers, Alfred (1892). Photography: its history, processes. London: Griffin. paragraph 257. OCLC 558063884.
- Svrcek, Mirko (1975). A color guide to familiar mushrooms (2nd ed.). London: Octopus Books. paragraph 30. ISBN 0-7064-0448-3.
- Accum, Friedrich (1820). A Treatise on Food Adulteration and Culinary Poisons: A Demonstration of the Fraudulent Sophistications of Bread, Beer, Wine, Spirits, Tea, Coffee, Cream, Confectionery, Vinegar, Mustard, Pepper, Cheese, Olive Oil, Pickles and Other Items Used in the Domestic Economy and methods for their identification. Chemical plant Mallinckrodt. pp. 133–134.
- https://www.mindat.org/min-3469.html
- https://www.mindat.org/min-3643.html
- https://www.mindat.org/min-1517.html
- https://www.mindat.org/min-2633.html
- https://www.mindat.org/min-1124.html
- Wildermuth, Egon; Stark, Hans; Friedrich, Gabriele; Ebenhoch, Franz Ludwig; Cubort, Bridget; Silver, Jack; Rituper, Rafael. "Iron compounds". Ullman Encyclopedia of Industrial Chemistry
. Weinheim: Wiley-VCH. - Price, William (1778). Mineralogia Cornubiensis; A Treatise on Minerals, Mines and Mining. London: Phillips. paragraph 33.
What is this substance?
Iron sulfate is an inorganic substance, a compound of sulfuric acid and iron salt, colorless, opaque, odorless. Crystal hydrates have a pale bluish-green color and are transparent, tetrahydrates (FeSO4 4H2O) are green in color, and monohydrates (FeSO4 H2O) are colorless. The substance tastes sharply astringent, with a metallic aftertaste. From the name it is clear that it has a strong acid component, the molar mass of the reagent is 151 g/mol. The formula of iron sulfate is FeSO4.
In air, the substance evaporates, losing the crystallization liquid in the process. The compound dissolves quickly in water at a temperature of 20 °C. Its toxicity is relatively low. Of the liquid mixtures, only bluish-green heptahydrate, better known as iron sulfate (FeSO4 7H2O), has the ability to crystallize. Thanks to its properties, the substance is used in chemistry lessons, showing students how unusual crystals can be grown from it in a short time.
Application in viticulture
Many summer residents are trying to grow grape crops on their property. At the same time, the shrub bears fruit well not only in the southern regions of the country, but also in the middle zone. If you provide it with proper care, you can reap a good harvest. The main secret of experienced gardeners is to spray the vineyards with iron sulfate in the fall. With its help you can resist the attack of harmful bacteria and various microorganisms. You should not spare the nutrient solution of iron sulfate; you need to spray the vine with it quite strongly, and also treat the soil around the grape bush, since pests can breed in it.
The use of iron sulfate in the vineyard is also effective in the spring. This feeding will allow the plant to more easily tolerate possible frosts. In addition, treatment with the solution will slightly inhibit bud growth. That is why it is important to spray before the first leaves appear. In addition, if a highly concentrated liquid solution gets on them, burns will form.
Before planting the cuttings in the ground, it is also a good idea to moisten them with a solution of iron sulfate. It is prepared in the same way as for spraying. This treatment will allow the cuttings to take root and germinate faster. The composition retains its beneficial properties for three months from the date of preparation.
Application in agriculture
Iron sulfate has also found its use in agriculture. Farmers especially widely use iron sulfate as a fungicide to combat numerous fungal diseases to which plants are susceptible. Moreover, it is used to disinfect the walls of basements and vegetable stores.
A solution of ferrous sulfate is used on an ongoing basis for seed treatment. In this way, they are prevented from becoming infected with harmful microorganisms, germination is increased and infection of other crops is prevented. It is important to note the undeniable benefits of iron sulfate as an effective fertilizer for certain types of soils and crops.
Receipt
In industry, iron (III) sulfate is obtained by calcining pyrite or marcasite with NaCl in air:
2FeS2 + 2NaCl + 8O2 ⟶ Fe2(SO4)3 + Na2SO4 + Cl2
or dissolve iron (III) oxide in sulfuric acid:
Fe2O3 + 3H2SO4 ⟶ Fe2(SO4)3 + 3H2O
In laboratory practice, iron (III) sulfate can be obtained from iron (III) hydroxide:
2Fe(OH)3 + 3H2SO4 ⟶ Fe2(SO4)3 + 6H2O
A preparation of the same purity can be obtained by oxidation of iron (II) sulfate with nitric acid:
2FeSO4 + H2SO4 + 2 HNO3 ⟶ Fe2(SO4)3 + 2NO2 + 2H2O
oxidation can also be carried out with oxygen or sulfur oxide:
12FeSO4 + 3O2 ⟶ 4Fe2(SO4)3 + 2Fe2O3 2FeSO4 + 2SO3 ⟶ Fe2(SO4)3 + SO2
Concentrated sulfuric and nitric acids oxidize iron sulfide to iron (III) sulfate:
2FeS + H2SO4 + 18HNO3 ⟶ Fe2(SO4)3 + 18NO2↑ + 10H2O
Iron disulfide can be oxidized with concentrated sulfuric acid:
2FeS2 + 14H2SO4 ⟶ Fe2(SO4)3 + 15SO2↑ + 14H2O
Iron(II) ammonium sulfate (Mohr's salt) can also be oxidized with potassium dichromate. As a result of this reaction, four sulfates are released at once - iron (III), chromium (III), ammonium and potassium, and water:
6Fe(NH4)2(SO4)2 + 7H2SO4 + K2Cr2O7 ⟶ Fe2(SO4)3 + Cr2(SO4)3 + 6(NH4)2SO4 + K2SO4 + 7H2O
Iron (III) sulfate can be obtained as one of the products of the thermal decomposition of iron (II) sulfate:
6FeSO4 →T Fe2(SO4)3 + 2Fe2O3 + 3SO2
Ferrates are reduced with dilute sulfuric acid to iron (III) sulfate:
4K2FeO4 + 10H2SO4 → 2Fe2(SO4)3 + 3O2↑ + 4K2SO4 + 10H2O
When the pentahydrate is heated to a temperature of 70–175 °C, anhydrous iron (III) sulfate is obtained:
Fe2(SO4)3 ⋅ 5H2O →70−175oC Fe2(SO4)3 + 5H2O
Iron(II) sulfate can be oxidized with xenon trioxide:
XeO3 + 3H2SO4 + 6FeSO4 ⟶ 3Fe2(SO4)3 + Xe↑ + 3H2O
Maltofer
Release forms for oral administration: drops, syrup, chewable tablets.
Main feature: iron hydroxide is combined with carbohydrates. This complex is called: “Iron hydroxide polymaltosate.” In articles and instructions it is referred to by the abbreviation HPC (hydroxide-polymaltose complex).
Its structure is similar to that of the natural iron compound ferritin. Thanks to this, it can connect with the transport protein, which delivers iron from the intestines to the blood.
GPC is stable. “pure” iron is not released into the gastrointestinal tract, and therefore there are significantly fewer adverse reactions when using it.
Pregnant and breastfeeding women can. Maltofer Fol will be optimal , which contains folic acid necessary for normal growth and development of the fetus.
Children: Maltofer drops, syrup - from birth, tablets - from 12 years.
Adverse reactions: nausea, constipation, diarrhea, dark stool, rash, itching, discoloration of tooth enamel.
Drug interactions - no.
There are no food interactions.
How to take: for the treatment of IDA, adults take 40-120 drops or 10-30 ml of syrup or 1-3 tablets per day. (100-300 mg pure iron) during or after meals. Chewable tablets can be swallowed as usual.
Maltofer in the form of drops or syrup can be mixed with fruit juice, vegetable puree, and milk mixture.
Ferrum Lek
Ferrum Lek used to be almost the only iron preparation for parenteral administration. There were no oral forms of it.
And now they are: syrup and chewable tablets.
Ferrum Lek is an analogue of the drug Maltofer in the form of syrup and chewable tablets. So, if something happens, they can replace Maltofer.
How to take: for adults to treat IDA, 10-30 ml of syrup (100-300 mg of iron) or 1-3 tablets per day during or after meals. After hemoglobin returns to normal, continue taking the drug 1 tablet until ferritin (iron reserves) normalizes.
