Magnesium sulfate is a white, orthorhombic crystal that has a density of 2.66 grams per mL and a melting point of 1,124 degC. This hygroscopic, odorless compound is used in fireproofing, textile processes, ceramics, and fertilizers.
This ionic compound is neutrally charged with a magnesium cation and a sulfate anion. The cation consists of two sulphur-oxygen double bonds, while the sulfate anion consists of four oxygen atoms that singly bond with each other.
Hydrolysis of magnesium sulfate into sulfates and bicarbonates is an important chemical process in natural water systems. Hydrated magnesium sulfate forms up to 1/6 of the mass of carbonaceous chondrites and is probably an important solute in cryovolcanic brines erupted on certain icy objects in the outer solar system.
Molecular Equilibria at Elevated Pressures
When this sulfate is dissolved in water, the magnesium cation and the sulfate anion become dissociated. The sulfate anion becomes neutrally charged with an ionic charge of +2 because the sulphur-oxygen double bonds cancel each other out, while the single oxygen atoms singly bond each other to form a negative charge of -1.
During thermal decomposition, MGS-CAP and PA-CAP samples exhibit oxidation and chlorination of the phthalic acid. The resulting products release sulfur- and chlorine-bearing species, HCl, SO2, and linear alkene around 450 to 550degC (Figures 1b and 2c, red lines).
In addition to its anticonvulsant properties, magnesium sulfate is an important tocolytic. Its mechanism of action is unclear but is thought to be the inhibition of chorioamnionitis inflammation. It has also been shown to modulate the augmented IL-1I2 response triggered by LPS and viral dsRNA. It is therefore possible that it has a broader therapeutic application.