Sodium Sulfate

Sodium Sulfate

Sodium sulfate (Na2SO4) is the sodium salt of sulfuric acid. Anhydrous sulfate is a white crystalline solid also known as the mineral thenardite, while the decahydrate Na2SO4.10H2O has been known as Glauber’s salt or mirabilis. Na2SO4.7H2O is transformed to mirabilite when it is cooled. Mirabilite is the natural mineral form of the decahydrate. About two-thirds of the world’s production of sodium sulfate is obtained from mirabilite. It is also produced from by-products of chemical processes such as hydrochloric acid production.

In 1625, Johann Rudolf Glauber discovered the sodium sulfate from Austrian spring water, there so the hydrate form is known as Glauber’s salt. Due to its medicinal properties, he named it as sal mirabilis (miraculous salt). The crystals were used as a general purpose laxative, until the 1900s. By reaction with potassium carbonate or potash, Glauber’s salt was used as a raw material for the industrial production of soda ash in the 18th century. In the nineteenth century the demand of soda ash was increased, so the large scale Leblanc process which produced synthetic sodium sulfate became the principal method of soda ash production.

At dietary levels, excretion is mainly in the urine. Sulfates are found in all body cells, with highest concentrations in connective tissues, bone, and cartilage. Sulfates play a role in several important metabolic pathways, including those involved in detoxification processes.

There are two types of sodium sulphate natural and byproduct, also known as synthetic. Natural sodium sulfate is produced from naturally occurring brines and crystalline deposits found in California and Texas. It is also found as a constituent of saline lakes, such as the Great Salt Lake in Utah. Synthetic sodium sulfate is recovered as a byproduct from various manufacturing processes. Both types of sodium sulfate have several important and useful applications in various consumer products. In a survey of the top 50 basic organic and inorganic chemicals made in the United States, sodium sulfate ranked 47th in terms of quantity produced.

Resources

Sodium is the sixth most abundant element in the Earth’s crust. Sodium sulfate-bearing mineral deposits are geologically young, mainly of post-glacial age. Sodium sulfate is widespread in occurrence and is a common component of seawater and many saline or alkaline lakes. Economic reserves of natural sodium sulfate are estimated at 3.3 billion tons worldwide. With world production of natural sodium sulfate averaging about 2.6 million tons per year, supplies are sufficient to meet anticipated demand for several centuries. The quantity of synthetic sodium sulfate is dependent on the longevity of the manufacturing firms recovering byproduct sulfate.

Surface depressions or lakes that have no outlets and are fed by spring waters flowing over volcanic rocks containing sulfide minerals often yield soluble sulfide salts that are oxidized by contact with the air to produce sulfates.

Properties

Molecular formula Na2SO4
Molecular weight 142.04gm/mole (anhydrous), 322.20gm /mole (decahydrate)
Appearance White crystalline solid
Odour Odourless
Boiling point 14290C(anhydrous)
Flashpoint 8000C
Melting point 8840 C (anhydrous), 32.40C (decahydrate)
Density 2.664gm/ml (anhydrous), 1.464gm/ml (decahydrate)
Refractive index 1.468 (anhydrous), 1.394 (decahydrate)
Solubility Soluble in water, glycerol and
hydrogen iodide and insoluble in
ethanol

Uses of Sodium Sulphate

  • Sodium sulfate is used to dry organic liquids.
  • As a filler in powdered home laundry detergents.
  • As a fining agent which removes small air bubbles from molten glass.
  • Glauber’s salt, the decahydrate was used as a laxative which removes the certain drugs such as acetaminophen from the body.
  • For defrosting windows, in carpet fresheners, starch manufacture, as an additive to cattle feed.
  • In the manufacture of detergents and in the Kraft process of paper pulping.

Practise This Question

Which of the following is the first step performed in the purification of river water?