Magnesium sulfate is an inorganic salt and compound of chemistry. It contains magnesium, sulfur, and oxygen. The primary medical use of sulfate was in 1618. It’s on the World Health Organization’s List of Essential Medicines because of the safest and best medicines needed during a health system. A farmer in Epsom, England discovered the sulfate. When Epsom’s cows refused to drink the water from a particular mineral well, he tasted the water and located that it tasted very bitter. This incident inspired Epsom to get sulfate. During this chapter, we’ll study Magnesium Sulfate Formula and its different applications.
Magnesium Sulfate Formula
Magnesium sulfate may be a magnesium salt having sulfate because of the counterion. It’s a task as an anticonvulsant, a cardiovascular drug, and a calcium channel blocker. Also, it’s used as an anesthetic, a tocolytic agent, an anti-arrhythmia drug and an analgesic. It’s a magnesium salt and a metal sulfate. Athletes use it to appease sore muscles, while gardeners use it to enhance crops.
- Molecular Magnesium Sulfate Formula= MgSO4
- The molecular formula of Epsom salt = MgSO 4· 7H2O
- IUPAC name= Magnesium sulfate
- The Simplified molecular-input line-entry system (SMILES) = [O-]S(=O)(=O)[O-].[Mg+2]
- The most common magnesium sulfate is heptahydrate sulfate mineral epsomite (MgSO4·7H2O).
In agriculture, sulfate is used to extend magnesium or sulfur content within the soil. The advantage of sulfate over other magnesium soil amendments (such as dolomitic lime) is its high solubility. It also allows for the choice of foliar feeding. Brewing salt in making beer is another use of it. Anhydrous sulfate is usually used as a desiccant in organic synthesis because of its affinity for water and compatibility with most organic compounds.
Preparation of Magnesium Sulfate
Magnesium sulfate is often prepared within the laboratory. First of all, Dissolution of periclase, magnesium hydroxide or magnesium carbonate in dilute vitriol. Then evaporation of the resulting solution when sulfate heptahydrate crystallizes MgSO4, 7H2O crystallizes out.
The monohydrate, MgSO4·H2O is that the mineral kieserite. Heating the hexahydrate to approximately 150 °C forms the monohydrate. Further heating to approximately 200 °C gives anhydrous sulfate. Upon further heating, the anhydrous salt decomposes into magnesia (MgO) and sulfur trioxide (SO3). The heptahydrate is often prepared by neutralizing vitriol with magnesium carbonate or oxide. But it’s usually obtained directly from natural sources.
MgCO3 + (NH4)2SO4(conc.) ⇒ MgSO4 + 2NH3↑ + CO2↑ + H2O (boiling).
Solved Examples for Magnesium Sulfate Formula
Q1] Discuss different reactions to form magnesium sulfate with the action of sulfuric acid on magnesium oxide, hydroxide, or carbonate.
Solution – In the laboratory, with the help of evaporation and crystallization, magnesium sulfate is formed.
MgO + H2SO4 ⇒ MgSO4 + H2O
Mg(OH)2 + H2SO4 ⇒ MgSO4 + 2H2O
MgCO3 + H2SO4 ⇒ 4 + CO2 + H2O
Q2] Write chemical reactions with Magnesium sulfate over different temperatures.
Solution – MgSO4 • 7H2O ⇒ MgSO4 + 7H2O (200-330° C).
MgSO4 + H2SO4(conc. cold) ⇒ Mg(HSO4)2.
MgSO4 + 2NaOH(diluted) ⇒ Mg(OH)2↓ + Na2SO4.
MgSO4 + 2KHCO3 ⇒ MgCO3↓ + K2SO4 + H2O + CO2↑
2MgSO4 + H2O + 2Na2CO3 ⇒ Mg2CO3(OH)2↓ + 2Na2SO4 + CO2↑ (boiling).
MgSO4(saturated) + CaCrO4(saturated) ⇒ MgCrO4 + CaSO4↓.
2MgSO4 ⇒ 2MgO + 2SO2 + O2 (over 1200° C).