Sodium sulfate

Absorption

Absorption of sodium sulfate after ingestion in rats was investigated. 35)S-Radioactivity excreted in urine during 24 hr indicated almost complete absorption from GI tract. Determination in serum 2 hr after admin revealed 3-fold increase in sulfate concentration rapid and almost complete absorption of inorganic sulfate occurs after oral admin in rats.

Description

Anhydrous sodium sulfate (Na2SO4) is typically used in organic chemistry as a drying agent. After aqueous extractions the organic layer always has a certain amount of water left in it. Adding anhydrous sodium sulfate removes this water by forming the sodium sulfate hydrate, which conveniently is also a solid allowing it to be filtered away. Magnesium sulfate (MgSO4) is a similar drying agent.

Chemical properties

Sodium sulfate, also known as thenardite and salt cake, is a crystalline compound that melts at 888°C (1632°C). Sodium sulfate is found in natural form(thenardite) in Chile and Spain. It is used in the manufacture of paperboard, glass,and freezing mixtures. It is used in dyeing,manufacturing glass,and in the preparation of sodium bisulfate.

Physical properties

Sodium sulfate is a white crystalline solid. It frequently is found as the decahydrate. orthorhombic or hexagonal structure; hygroscopic; refractive index 1.468; hardness 2.8 Mohs; density 2.664 g/cm3; melts at 884°C; soluble in water, insoluble in ethanol. The decahydrate consists of colorless monoclinic crystals; refractive index 1.394; hardness 1.8 Mohs; density 1.4 6g/cm3; decomposes at 32°C; soluble in water; insoluble in ethanol.

Occurrence

Sodium sulfate occurs in nature as the minerals mirabilite and thenardite. While thenardite is the anhydrous form of Na₂SO₄, mirabilite is a naturallyoccurring decahydrate, Na₂SO₄.10H₂O.
Sodium sulfate is one of the most important sodium salts. The decahydrate,commonly known as the Glauber’s salt, was first prepared by Johann Glauber in the seventeenth century as a by-product in making hydrochloric acid from sulfuric acid and sodium chloride.

The Uses of Sodium sulfate

Sodium sulfate serves several functions in industrial and laboratory settings. In the manufacturing of synthetic detergents and soaps, it is primarily used as a filler. It is also a common laboratory reagent, where its principal application is as a drying agent to remove residual water from organic solvents and their extracts. Additionally, sodium sulfate is utilized as a starting material for the chemical synthesis of other sodium salts.

Background

Sodium Sulfate Anhydrous is the anhydrous, sodium salt form of sulfuric acid. Sodium sulfate anhydrous disassociates in water to provide sodium ions and sulfate ions. Sodium ion is the principal cation of the extracellular fluid and plays a large part in the therapy of fluid and electrolyte disturbances. Sodium sulfate anhydrous is an electrolyte replenisher and is used in isosmotic solutions so that administration does not disturb normal electrolyte balance and does not lead to absorption or excretion of water and ions.

Indications

indicated for bowel cleansing prior to colonoscopy or barium enema X-ray examination.

Production Methods

Sodium sulfate can be produced industrially through two primary methods. The first involves the reaction of magnesium sulfate with sodium chloride in solution, followed by crystallization. The second method is the reaction of concentrated sulfuric acid with solid sodium chloride. This latter process was integral to the historic Leblanc process for alkali production and is the origin of the term "salt cake" for impure, industrial-grade sodium sulfate. Industrially, sodium sulfate is used in the manufacturing of glass and soft glazes. In the dyeing industry, it is employed as a leveling agent to promote an even finish. It also has medicinal applications as a laxative and is a component of some commercial purgative salts.

Pharmacokinetics

Induces catharsis by the osmotic effects of the unabsorbed sulfate salts and polyethylene glycol (PEG) in the GI tract. Specifically, sulfate salts provide sulfate anions, which are poorly absorbed, and PEG, which is primarily unabsorbed, causes water to be retained in the GI tract resulting in watery diarrhea.

Toxicity

Moderately toxic by intravenous route. Mildly toxic by ingestion. An experimental teratogen. Experimental reproductive effects. Questionable carcinogen with experimental tumorigenic effects. Violent reaction with Al. When heated to decomposition it emits toxic fumes of SOx and Na2O. 

Potential Exposure

Sodium sulfate is used in the manufacture of glass; as a precipitating agent in the manufacture of silver emulsions; as an analytical reagent; in making ultramarine and paper pulp; in ceramic glazes and pharmaceuticals; as a food additive; and a filler in synthetic detergents.

Chemical property

Hygroscopic. Sodium sulfate reacts violently with magnesium. Also incompatible with aluminum, potassium, mercury, lead, calcium, silver, barium, ammonium ions, and strontium. Sulfates give precipitates with salts of lead, barium, strontium, and calcium. Silver and mercury form slightly soluble salts. Alcohol preciptates most sulfates out of solution.

Incompatibilities

Violent reaction with aluminum, magnesium. Attacks metals in the presence of moisture.

Waste Disposal

Do not discharge waste sodium sulfate directly into sewers or surface waters. Recovered sodium sulfate may be disposed of by burial in a landfill.