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Sodium sulfate (also known as sodium sulphate or sulfate of soda) is the inorganic compound with formula Na2SO4 as well as several related hydrates.
Sodium sulfate is used primarily for drying non-aqueous solvents by removing traces of water.
Sodium sulfate is defined as the sodium salt of sulfuric acid.
CAS number: 7757-82-6
EC number: 231-820-9
Molecular Formula: Na2O4S
Molecular Weight (g/mol): 142.04
With an annual production of 6 million tonnes, the decahydrate is a major commodity Sodium sulfate.
Sodium sulfate is mainly used as a filler in the manufacture of powdered home laundry detergents and in the Kraft process of paper pulping for making highly alkaline sulfides.
Sodium sulfate is used primarily for drying non-aqueous solvents by removing traces of water.
Sodium sulfate is used as a fining agent for molten glass, levelling agent in textile processing, and filler in detergents.
Sodium sulfate is also used in Kraft process for paper pulping, defrosting windows, manufacture of starch, glass, and soap.
Sodium sulfate is an inorganic sodium salt.
Sodium Sulfate is the sodium salt form of sulfuric acid.
Sodium sulfate 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 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.
Sodium sulfate (also known as sodium sulphate or sulfate of soda) is the inorganic compound with formula Na2SO4 as well as several related hydrates.
All forms are white solids that are highly soluble in water.
Sodium sulfate is defined as the sodium salt of sulfuric acid.
The sodium sulfate chemical formula is Na2SO4.
Anhydrous sulfate can be described as a white crystalline solid, which is also called mineral thenardite, whereas, the decahydrate Na2SO4.10H2O has been called either mirabilis or Glauber's salt.
When Na2SO4.7H2O is cooled, Sodium sulfate is transformed to mirabilite, which is the natural mineral form of decahydrate.
About two-thirds of the sodium sulfate's world's production is obtained from mirabilite.
Sodium sulfate is also formed from the by-products of chemical processes like hydrochloric acid production.
Sodium sulfate is a neutral salt, Sodium sulfate can be obtained mostly in lakes with brackish and salty water, in mineral deposits present in solid form, and as a chemical by-product.
Natural sodium sulfate does not contain any zinc, arsenic, other heavy metals such as lead and chromium, and toxic minerals.
Sodium sulfate is preferred in many sectors as an additive in the production of suitable products, both in natural and synthetic form.
Sodium sulfate is found in sodium sulfate (Na2SO4) compounds that are available in nature.
Sodium sulfate is ready for use after processing and evaluation of dissolved liquids and other raw materials of mineral ores in solid form of sodium sulfate, which is found as solid in this way.
Sodium sulfate, which is used as a main ingredient in industries, is preferred because Sodium sulfate is a neutral salt.
In general, the reason why sodium sulfate is usable in the industry is that Sodium sulfate is used because Sodium sulfate is not similar to other water-soluble substances.
Generally, sodium sulfate is supplied from completely natural sources as well as in the form of another by-product, synthetic sodium sulfate, as a result of being included in the materials.
In sodium sulfate, which is mostly produced synthetically, Sodium sulfate main production residues remain, albeit in very small amounts.
Forms of Sodium Sulfate:
Anhydrous sodium sulfate, known as the rare mineral thenardite, used as a drying agent in organic synthesis.
Heptahydrate sodium sulfate, a very rare form.
Decahydrate sodium sulfate, known as the mineral mirabilite, widely used by chemical industry.
Sodium sulfate is also known as Glauber's salt.
Uses of Sodium Sulfate:
In 1995, bulk sodium sulfate sold for around $70 per tonne in the US, making Sodium sulfate a very cheap material.
Probably the largest use for sodium sulfate today is as a filler in powdered home laundry detergents.
Total consumption of Na2SO4 in Europe was around 1.6 million tonnes in 2001, of which 80% was used for detergents.
However this use is waning as domestic consumers are increasingly switching to liquid detergents that do not include the chemical.
Another major use for Na2SO4, particularly in the US, is in the Kraft process for the manufacture of wood pulp.
Organics present in the "black liquor" from this process are burnt to produce heat, needed to drive the reduction of sodium sulfate to sodium sulfide.
However, this process is being replaced to some extent by newer processes; use of Na2SO4 in the US pulp industry declined from 980 000 tonnes in 1970 to only 210 000 tonnes in 1990.
The glass industry also provides another significant application for sodium sulfate, consuming around 30 000 tonnes in the US in 1990 (4% of total US consumption).
Sodium sulfate is used as a "fining agent", to help remove small air bubbles from molten glass.
Sodium sulfate also fluxes the glass, and prevents scum formation of the glass melt during refining.
Sodium sulfate is important in the manufacture of textiles, particularly in Japan.
Sodium sulfate helps in "levelling", reducing negative charges on fibres so that dyes can penetrate evenly.
Unlike the alternative sodium chloride, Sodium sulfate does not corrode the stainless steel vessels used in dyeing.
Glauber's salt, the decahydrate, was formerly used as a laxative.
Sodium sulfate has also been proposed for heat storage in passive solar heating systems.
This takes advantage of the unusual solubility properties (see above), and the high heat of crystallisation (78.2 kJ/mol).
Other uses for sodium sulfate include frosting windows, in carpet fresheners, starch manufacture and as an additive to cattle feed.
In the laboratory, anhydrous sodium sulfate is widely used as an inert drying agent for organic solutions; Na2SO4 is added to the solution until the crystals no longer clump together.
Sodium sulfate is used to dry organic liquids.
Sodium sulfate is used as a filler in powdered home laundry detergents.
Sodium sulfate is used as a fining agent which removes small air bubbles from molten glass.
Glauber’s salt, the decahydrate, was used as a laxative which removes certain drugs such as acetaminophen from the body.
For defrosting windows, in carpet fresheners, starch manufactured, as an additive to cattle feed.
In the manufacture of detergents and in the Kraft process of paper pulping.
Sodium sulfate is used for standardizing dyes; in freezing mixtures; in dying and printing textiles.
Sodium sulfate is produced from mineral deposits and may contain the following contaminants: dichromate (less than 0.2%), sodium sulfite, sodium chloride, magnesium chloride, magnesium sulfate, lithium carbonate, lithium sulfate, ferric oxide, cupric chloride, sodium hydrogen sulfate, sodium thiosulfate, and boric acid;
Industry Uses:
Adhesives and sealant chemicals
Anti-scaling agent
Bleaching agents
Brightener
Catalyst
Cleaning agent
Dye
Dyes
Filler
Fillers
Flocculating agent
Functional fluids (closed systems)
Intermediate
Intermediates
Laboratory chemicals
Lubricating agent
Not Known or Reasonably Ascertainable
Other
Other (specify)
Oxidizing/reducing agents
Paint additives and coating additives not described by other categories
Pigment
Pigments
Process regulators
Processing aids not otherwise specified
Processing aids, not otherwise listed
Processing aids, specific to petroleum production
Softener and conditioner
Soil amendments (fertilizers)
Solids separation (precipitating) agent, not otherwise specified
Solids separation agents
Solvents (which become part of product formulation or mixture)
Stabilizing agent
Surface active agents
Surfactant (surface active agent)
Tanning agents not otherwise specified
Thickening agent
Waterproofing agent
pH regulating agent
Consumer Uses:
Adhesives and sealant chemicals
Dehydrating agent (desiccant)
Dye
Filler
Fillers
Functional fluids (closed systems)
Intermediate
Laboratory chemicals
Not Known or Reasonably Ascertainable
Other
Other (specify)
Paint additives and coating additives not described by other categories
Pigment
Pigments
Processing aids not otherwise specified
Processing aids, not otherwise listed
Softener and conditioner
Surface active agents
Surfactant (surface active agent)
Thickening agent
Industrial Processes with risk of exposure:
Mining
Textiles (Printing, Dyeing, or Finishing)
Activities with risk of exposure:
Textile arts
Usage Areas of Sodium Sulfate:
The paper industry is a very important chemical substance used by cooking fiber, especially in the manufacture of cellulose and sodium sulfate, which are the most important materials of paper.
Detergent industry, the first preferred area of use for sodium sulfate is the detergent industry.
Because sodium sulfate is present as a filler in the formula of solid detergents and powder granules.
Sodium sulfate, which is usually present in detergents, is around 16%, but in some cases this ratio can be around 40%.
The glass industry, especially in the creation of glass material, the biggest role belongs to sodium sulfate.
Textile dyeing mostly helps the sodium sulfate dye to pass into the fabric completely homogeneously in this area.
Sodium sulfate is the most important chemical used in the cooking of fiber in the manufacture of cellulose in the paper industry.
Sodium sulfate is used at a rate of 25% in the detergent industry.
Since Sodium sulfate does not contain any toxic substances and obtaining a natural pH value, Sodium sulfate is of great importance in this sector.
Sodium sulfate is used as a filler in the detergent industry.
Sodium sulfate is used in the formation of frit in the glass industry.
Sodium sulfate is consumed at the rate of 3% in glass production.
In textile dyeing, Sodium sulfate provides a homogeneous transfer of the dye to the textile surface.
Sodium sulfate is used in the chemical industry to obtain chemicals such as potassium sulfate, aluminum sulfate, sodium silicate, sodium sulfide.
Applications of Sodium Sulfate:
Sodium sulfate is used primarily for drying non-aqueous solvents by removing traces of water.
Sodium sulfate is used as a fining agent for molten glass, levelling agent in textile processing, and filler in detergents.
Sodium sulfate is also used in Kraft process for paper pulping, defrosting windows, manufacture of starch, glass, and soap.
Commodity industries:
With US pricing at $30 per tonne in 1970, up to $90 per tonne for salt cake quality, and $130 for better grades, sodium sulfate is a very cheap material.
The largest use is as filler in powdered home laundry detergents, consuming approximately 50% of world production.
This use is waning as domestic consumers are increasingly switching to compact or liquid detergents that do not include sodium sulfate.
Papermaking:
Another formerly major use for sodium sulfate, notably in the US and Canada, is in the Kraft process for the manufacture of wood pulp.
Organics present in the "black liquor" from this process are burnt to produce heat, needed to drive the reduction of sodium sulfate to sodium sulfide.
However, due to advances in the thermal efficiency of the Kraft recovery process in the early 1960s, more efficient sulfur recovery was achieved and the need for sodium sulfate makeup was drastically reduced.
Hence, the use of sodium sulfate in the US and Canadian pulp industry declined from 1,400,000 tonnes per year in 1970 to only approx. 150,000 tonnes in 2006.
Glassmaking:
The glass industry provides another significant application for sodium sulfate, as second largest application in Europe.
Sodium sulfate is used as a fining agent, to help remove small air bubbles from molten glass.
Sodium sulfate fluxes the glass, and prevents scum formation of the glass melt during refining.
The glass industry in Europe has been consuming from 1970 to 2006 a stable 110,000 tonnes annually.
Textiles:
Sodium sulfate is important in the manufacture of textiles, particularly in Japan, where this is the largest application.
Sodium sulfate is added to increase the ionic strength of the solution and so helps in "levelling", i.e. reducing negative electrical charges on textile fibres, so that dyes can penetrate evenly (see the theory of the diffuse double layer (DDL) elaborated by Gouy and Chapman).
Unlike the alternative sodium chloride, Sodium sulfate does not corrode the stainless steel vessels used in dyeing.
This application in Japan and US consumed in 2006 approximately 100,000 tonnes.
Food industry:
Sodium sulfate is used as a diluent for food colours.
Sodium sulfate is known as E number additive E514.
Heat storage:
The high heat-storage capacity in the phase change from solid to liquid, and the advantageous phase change temperature of 32 °C (90 °F) makes Sodium sulfate especially appropriate for storing low-grade solar heat for later release in space heating applications.
In some applications Sodium sulfate is incorporated into thermal tiles that are placed in an attic space, while in other applications, the salt is incorporated into cells surrounded by solar–heated water.
The phase change allows a substantial reduction in the mass of Sodium sulfate required for effective heat storage (the heat of fusion of sodium sulfate decahydrate is 82 kJ/mol or 252 kJ/kg), with the further advantage of a consistency of temperature as long as sufficient material in the appropriate phase is available.
For cooling applications, a mixture with common sodium chloride salt (NaCl) lowers the melting point to 18 °C (64 °F).
The heat of fusion of NaCl·Na2SO4·10H2O, is actually increased slightly to 286 kJ/kg.
Small-scale applications:
In the laboratory, anhydrous sodium sulfate is widely used as an inert drying agent, for removing traces of water from organic solutions.
Sodium sulfate is more efficient, but slower-acting, than the similar agent magnesium sulfate.
Sodium sulfate is only effective below about 30 °C, but Sodium sulfate can be used with a variety of materials since Sodium sulfate is chemically fairly inert.
Sodium sulfate is added to the solution until the crystals no longer clump together; the two video clips (see above) demonstrate how the crystals clump when still wet, but some crystals flow freely once a sample is dry.
Glauber's salt, the decahydrate, is used as a laxative.
Sodium sulfate is effective for the removal of certain drugs, such as paracetamol (acetaminophen) from the body; thus Sodium sulfate can be used after an overdose.
In 1953, sodium sulfate was proposed for heat storage in passive solar heating systems.
This takes advantage of Sodium sulfate unusual solubility properties, and the high heat of crystallisation (78.2 kJ/mol).
Other uses for sodium sulfate include de-frosting windows, starch manufacture, as an additive in carpet fresheners, and as an additive to cattle feed.
At least one company, Thermaltake, makes a laptop computer chill mat (iXoft Notebook Cooler) using sodium sulfate decahydrate inside a quilted plastic pad.
Sodium sulfate slowly turns to liquid and recirculates, equalizing laptop temperature and acting as an insulation.
Discovery of Sodium Sulfate:
Johann Rudolf Glauber discovered the sodium sulfate in 1625 from Austrian spring water there the hydrate form is called Glauber's salt.
Because of Sodium sulfate medicinal properties, he named Sodium sulfate as sal mirabilis (which is otherwise called miraculous salt).
Preparations of Sodium Sulfate:
In 1625, Johann Rudolf Glauber discovered sodium sulfate from Austrian spring water, so Sodium sulfate hydrate form is known as Glauber’s salt.
Due to Sodium sulfate medicinal properties, he named Sodium sulfate sal mirabilis (miraculous salt).
One-third of the world’s sodium sulfate is produced as a by-product of other processes in the chemical industry.
Sodium sulfate is produced by the reaction of sodium chloride and sulphuric acid.
2 NaCl + H2SO4 → 2 HCl + Na2SO4
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 for soda ash 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 the 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 sulfate natural and by-product, also known as synthetic.
Natural sodium sulfate is produced from naturally occurring brines and crystalline deposits found in California and Texas.
Sodium sulfate is also found as a constituent of saline lakes, such as the Great Salt Lake in Utah.
Synthetic sodium sulfate is recovered as a by-product of 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.
Properties of Sodium Sulfate:
Chemical properties:
Sodium sulfate is a typical electrostatically bonded ionic sulfate.
The existence of free sulfate ions in solution is indicated by the easy formation of insoluble sulfates when these solutions are treated with Ba2+ or Pb2+ salts:
Na2SO4 + BaCl2 → 2 NaCl + BaSO4
Sodium sulfate is unreactive toward most oxidizing or reducing agents.
At high temperatures, Sodium sulfate can be converted to sodium sulfide by carbothermal reduction (aka thermo-chemical sulfate reduction (TSR), high temperature heating with charcoal, etc.):
Na2SO4 + 2 C → Na2S + 2 CO2
This reaction was employed in the Leblanc process, a defunct industrial route to sodium carbonate.
Sodium sulfate reacts with sulfuric acid to give the acid salt sodium bisulfate:
Na2SO4 + H2SO4 ⇌ 2 NaHSO4
Sodium sulfate displays a moderate tendency to form double salts.
The only alums formed with common trivalent metals are NaAl(SO4)2 (unstable above 39 °C) and NaCr(SO4)2, in contrast to potassium sulfate and ammonium sulfate which form many stable alums.
Double salts with some other alkali metal sulfates are known, including Na2SO4·3K2SO4 which occurs naturally as the mineral aphthitalite.
Formation of glaserite by reaction of sodium sulfate with potassium chloride has been used as the basis of a method for producing potassium sulfate, a fertiliser.
Other double salts include 3Na2SO4·CaSO4, 3Na2SO4·MgSO4 (vanthoffite) and NaF·Na2SO4.
Physical properties:
Sodium sulfate has unusual solubility characteristics in water.
Sodium sulfate solubility in water rises more than tenfold between 0 °C and 32.384 °C, where Sodium sulfate reaches a maximum of 49.7 g/100 mL.
At this point the solubility curve changes slope, and the solubility becomes almost independent of temperature.
This temperature of 32.384 °C, corresponding to the release of crystal water and melting of the hydrated salt, serves as an accurate temperature reference for thermometer calibration.
Resources of Sodium Sulfate:
Sodium is the sixth most abundant element in the Earth’s crust.
Sodium sulfate-bearing mineral deposits are geologically young, mainly of the 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 by-product sulfate.
Surface depressions or lakes that have no outlets and are fed by spring waters flowing over volcanic rocks containing sulphide minerals often yield soluble sulphide salts that are oxidised by contact with the air to produce sulfates.
Structure of Sodium Sulfate:
Crystals of the decahydrate consist of [Na(OH2)6]+ ions with octahedral molecular geometry.
These octahedra share edges such that 8 of the 10 water molecules are bound to sodium and 2 others are interstitial, being hydrogen-bonded to sulfate.
These cations are linked to the sulfate anions by hydrogen bonds.
The Na–O distances are about 240 pm.
Crystalline sodium sulfate decahydrate is also unusual among hydrated salts in having a measurable residual entropy (entropy at absolute zero) of 6.32 J/(K·mol).
This is ascribed to Sodium sulfate ability to distribute water much more rapidly compared to most hydrates.
Until the 1900s, the crystals present here were used as a general-purpose laxative, by reaction either with potash or potassium carbonate, where, in the 18th century, Glauber's salt was used as a raw material for the industrial production of soda ash.
In the 19thcentury, the demand for soda ash increased, so the large-scale Leblanc process which produced the synthetic sodium sulfate has become the principal method in the production of soda ash.
At dietary levels, the excretion is primarily in the urine.
Sulfates are found in the entire body cells, with the highest concentrations in bone, connective tissue, and cartilage.
Sulfates also play a major role in many important metabolic pathways, including those involved in the detoxification processes.
There exist two types of sodium sulfate natural and by-product, which is also called synthetic.
Natural sodium sulfate can be produced from naturally occurring crystalline deposits and brines, which are found in Texas and California.
Sodium sulfate is also found as a constituent of saline lakes, like the Great Salt Lake of Utah.
And, the synthetic sodium sulfate is recovered as a by-product of different manufacturing processes.
Both sodium sulfate types have many useful and important applications in different consumer products.
In a survey of the top 50 basic organic chemicals and inorganic chemicals performed in the United States, sodium sulfate has ranked 47th regarding the quantity produced.
Occurrence of Sodium Sulfate:
About half of the world's production of the decahydrate (Glauber's salt) is from the natural mineral form mirabilite - found in lake beds in southern Saskatchewan, for example.
In 1990, Mexico and Spain were the world's main producers of natural sodium sulfate (each around 500 000 tonnes), with USSR, USA and Canada also important (around 350 000 tonnes each).
Anhydrous sodium sulfate occurs in arid environments as the mineral thenardite, which is less common than mirabilite.
Sodium sulfate slowly turns to mirabilite in damp air.
Production of Sodium Sulfate:
The world production of sodium sulfate, almost exclusively in the form of the decahydrate, amounts to approximately 5.5 to 6 million tonnes annually (Mt/a).
In 1985, production was 4.5 Mt/a, half from natural sources, and half from chemical production.
After 2000, at a stable level until 2006, natural production had increased to 4 Mt/a, and chemical production decreased to 1.5 to 2 Mt/a, with a total of 5.5 to 6 Mt/a.
For all applications, naturally produced and chemically produced sodium sulfate are practically interchangeable.
Natural sources:
Two thirds of the world's production of the decahydrate (Glauber's salt) is from the natural mineral form mirabilite, for example as found in lake beds in southern Saskatchewan.
In 1990, Mexico and Spain were the world's main producers of natural sodium sulfate (each around 500,000 tonnes), with Russia, United States, and Canada around 350,000 tonnes each.
Natural resources are estimated at over 1 billion tonnes.
Major producers of 200,000 to 1,500,000 tonnes/year in 2006 included Searles Valley Minerals (California, US), Airborne Industrial Minerals (Saskatchewan, Canada), Química del Rey (Coahuila, Mexico), Minera de Santa Marta and Criaderos Minerales Y Derivados, also known as Grupo Crimidesa (Burgos, Spain), Minera de Santa Marta (Toledo, Spain), Sulquisa (Madrid, Spain), Chengdu Sanlian Tianquan Chemical (Tianquan County, Sichuan, China), Hongze Yinzhu Chemical Group (Hongze District, Jiangsu, China), Nafine Chemical Industry Group [zh] (Shanxi, China), Sichuan Province Chuanmei Mirabilite (万胜镇 [zh], Dongpo District, Meishan, Sichuan, China), and Kuchuksulphat JSC (Altai Krai, Siberia, Russia).
Anhydrous sodium sulfate occurs in arid environments as the mineral thenardite.
Sodium sulfate slowly turns to mirabilite in damp air.
Sodium sulfate is also found as glauberite, a calcium sodium sulfate mineral.
Both minerals are less common than mirabilite.
Chemical industry:
About one third of the world's sodium sulfate is produced as by-product of other processes in chemical industry.
Most of this production is chemically inherent to the primary process, and only marginally economical.
By effort of the industry, therefore, sodium sulfate production as by-product is declining.
The most important chemical sodium sulfate production is during hydrochloric acid production, either from sodium chloride (salt) and sulfuric acid, in the Mannheim process, or from sulfur dioxide in the Hargreaves process.
The resulting sodium sulfate from these processes is known as salt cake.
Mannheim: 2 NaCl + H2SO4 → 2 HCl + Na2SO4
Hargreaves: 4 NaCl + 2 SO2 + O2 + 2 H2O → 4 HCl + 2 Na2SO4
The second major production of sodium sulfate are the processes where surplus sodium hydroxide is neutralised by sulfuric acid to obtain sulfate (SO2−4) by using copper sulfate (CuSO4) (as applied on a large scale in the production of rayon by using copper(II) hydroxide).
This method is also a regularly applied and convenient laboratory preparation.
2 NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(l) ΔH=-112.5 kJ (highly exothermic)
In the laboratory Sodium sulfate can also be synthesized from the reaction between sodium bicarbonate and magnesium sulfate, by precipitating magnesium carbonate.
2 NaHCO3 + MgSO4 → Na2SO4 + MgCO3 + CO2 + H2O
However, as commercial sources are readily available, laboratory synthesis is not practised often.
Formerly, sodium sulfate was also a by-product of the manufacture of sodium dichromate, where sulfuric acid is added to sodium chromate solution forming sodium dichromate, or subsequently chromic acid.
Alternatively, sodium sulfate is or was formed in the production of lithium carbonate, chelating agents, resorcinol, ascorbic acid, silica pigments, nitric acid, and phenol.
Bulk sodium sulfate is usually purified via the decahydrate form, since the anhydrous form tends to attract iron compounds and organic compounds.
The anhydrous form is easily produced from the hydrated form by gentle warming.
Major sodium sulfate by-product producers of 50–80 Mt/a in 2006 include Elementis Chromium (chromium industry, Castle Hayne, NC, US), Lenzing AG (200 Mt/a, rayon industry, Lenzing, Austria), Addiseo (formerly Rhodia, methionine industry, Les Roches-Roussillon, France), Elementis (chromium industry, Stockton-on-Tees, UK), Shikoku Chemicals (Tokushima, Japan) and Visko-R (rayon industry, Russia).
Manufacturing Methods of Sodium Sulfate:
In Texas, subterranean sulfate brines are pumped to the surface where the brines are first saturated with NaCl before they are cooled by mechanical refrigeration to form Glauber's salt.
Sodium sulfate is then separated from Sodium sulfate mother liquor, melted, and dehydrated with mechanical vapor recompression evaporators.
Processing at Searles Lake, California, is similar to that of Texas brines.
Brine is cooled to 16 °C to remove borax crystals then cooled to 4 °C, which precipitates Glauber's salt.
Sodium sulfate is then separated from Sodium sulfate mother liquor, melted in multi-effect vacuum crystallizers to form anhydrous sodium sulfate, and dried.
Both processes produce crystals that are 99.3-99.7% pure.
The Mannheim process produces sodium sulfate by reaction of sodium chloride and sulfuric acid.
This reaction takes place in a fluidized-bed reactor or a specially made furnace called a Mannheim furnace.
This method was last used in the United States in the 1980s.
In another process, SO2, O2, and H2O react with NaCl.
This is called the Hargreaves process.
Only a minor amount of sodium sulfate is made in the United States using the Hargreaves process, but both the Hargreaves and the Mannheim processes are used widely in the rest of the world.
Sodium sulfate is prepared by the neutralization of sulfuric acid with sodium hydroxide.
General Manufacturing Information of Sodium Sulfate:
Industry Processing Sectors:
Agriculture, Forestry, Fishing and Hunting
All Other Basic Inorganic Chemical Manufacturing
All Other Basic Organic Chemical Manufacturing
All Other Chemical Product and Preparation Manufacturing
Construction
Electrical Equipment, Appliance, and Component Manufacturing
Food, beverage, and tobacco product manufacturing
Mining (except Oil and Gas) and support activities
Miscellaneous Manufacturing
Non-metallic Mineral Product Manufacturing (includes clay, glass, cement, concrete, lime, gypsum, and other non-metallic mineral product manufacturing)
Not Known or Reasonably Ascertainable
Oil and Gas Drilling, Extraction, and Support activities
Other (requires additional information)
Paint and Coating Manufacturing
Paper Manufacturing
Pesticide, Fertilizer, and Other Agricultural Chemical Manufacturing
Petrochemical Manufacturing
Petroleum Lubricating Oil and Grease Manufacturing
Petroleum Refineries
Pharmaceutical and Medicine Manufacturing
Primary Metal Manufacturing
Printing Ink Manufacturing
Printing and Related Support Activities
Services
Soap, Cleaning Compound, and Toilet Preparation Manufacturing
Textiles, apparel, and leather manufacturing
Transportation Equipment Manufacturing
Utilities
Wholesale and Retail Trade
Wood Product Manufacturing
History of Sodium Sulfate:
The decahydrate of sodium sulfate is known as Glauber's salt after the Dutch–German chemist and apothecary Johann Rudolf Glauber (1604–1670), who discovered Sodium sulfate in Austrian spring water in 1625.
He named Sodium sulfate sal mirabilis (miraculous salt), because of Sodium sulfate medicinal properties: the crystals were used as a general-purpose laxative, until more sophisticated alternatives came about in the 1900s.
In the 18th century, Glauber's salt began to be used as a raw material for the industrial production of soda ash (sodium carbonate), by reaction with potash (potassium carbonate).
Demand for soda ash increased, and the supply of sodium sulfate had to increase in line.
Therefore, in the 19th century, the large-scale Leblanc process, producing synthetic sodium sulfate as a key intermediate, became the principal method of soda-ash production.
Handling and Storage of Sodium Sulfate:
Storage Conditions:
Keep container tightly closed in a dry and well-ventilated place.
Keep well closed in a cool place.
Storage class (TRGS 510): Non Combustible Solids.
Safety of Sodium Sulfate:
Although sodium sulfate is generally regarded as non-toxic, Sodium sulfate should be handled with care.
The dust can cause temporary asthma or eye irritation; this risk can be prevented by using eye protection and a paper mask.
Transport is not limited, and no Risk Phrase or Safety Phrase applies.
Accidental Release Measures of Sodium Sulfate:
Personal protection:
Particulate filter respirator adapted to the airborne concentration of the substance.
Sweep spilled substance into covered containers.
If appropriate, moisten first to prevent dusting.
Cleanup Methods of Sodium Sulfate:
Personal precautions, protective equipment and emergency procedures:
Avoid dust formation.
Avoid breathing vapors, mist or gas.
Environmental precautions:
No special environmental precautions required.
Methods and materials for containment and cleaning up:
Sweep up and shovel.
Keep in suitable, closed containers for disposal.
Spills on land:
Contain if possible by forming mechanical barriers to prevent spreading.
Shovel material into containers for recovery or disposal.
Disposal Methods of Sodium Sulfate:
Recycle any unused portion of Sodium sulfate for Sodium sulfate approved use or return Sodium sulfate to the manufacturer or supplier.
Ultimate disposal of the chemical must consider:
Sodium sulfate's impact on air quality; potential migration in air, soil or water; effects on animal, aquatic and plant life; and conformance with environmental and public health regulations.
If Sodium sulfate is possible or reasonable use an alternative chemical product with less inherent propensity for occupational harm/injury/toxicity or environmental contamination.
Offer surplus and non-recyclable solutions to a licensed disposal company.
Contaminated packaging:
Dispose of as unused product.
Waste sodium sulfate must never be discharged directly into sewers or surface waters.
Recovered sodium sulfate may be disposed of by burial in a landfill.
Identifiers of Sodium Sulfate:
CAS Number:
7757-82-6
7727-73-3 (decahydrate)
ChEBI: CHEBI:32149
ChEMBL: ChEMBL233406
ChemSpider: 22844
ECHA InfoCard: 100.028.928
E number: E514(i) (acidity regulators, ...)
PubChem CID: 24436
RTECS number: WE1650000
UNII:
36KCS0R750
0YPR65R21J (decahydrate)
CompTox Dashboard (EPA): DTXSID102129
InChI: InChI=1S/2Na.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2
Key: PMZURENOXWZQFD-UHFFFAOYSA-L
InChI=1S/2Na.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2
InChI=1S/2Na.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2*+1;/p-2
Key: PMZURENOXWZQFD-UHFFFAOYSA-L
SMILES: [Na+].[Na+].[O-]S([O-])(=O)=O
CAS: 7757-82-6
Molecular Formula: Na2O4S
Molecular Weight (g/mol): 142.04
MDL Number: MFCD00003504
InChI Key: PMZURENOXWZQFD-UHFFFAOYSA-L
PubChem CID: 24436
ChEBI: CHEBI:32149
SMILES: [Na+].[Na+].[O-]S([O-])(=O)=O
CAS number: 7757-82-6
EC number: 231-820-9
Grade: ACS,ISO,Reag. Ph Eur
Hill Formula: Na₂O₄S
Chemical formula: Na₂SO₄
Molar Mass: 142.04 g/mol
HS Code: 2833 11 00
Quality Level: MQ300
Typical Properties of Sodium Sulfate:
Chemical formula: Na2SO4
Molar mass:
142.04 g/mol (anhydrous)
322.20 g/mol (decahydrate)
Appearance: white crystalline solid, hygroscopic
Odor: odorless
Density:
2.664 g/cm3 (anhydrous)
1.464 g/cm3 (decahydrate)
Melting point:
884 °C (1,623 °F; 1,157 K) (anhydrous)
32.38 °C (decahydrate)
Boiling point: 1,429 °C (2,604 °F; 1,702 K) (anhydrous)
Solubility in water: anhydrous:
4.76 g/100 mL (0 °C)
28.1 g/100 mL (25 °C)
42.7 g/100 mL (100 °C)
heptahydrate:
19.5 g/100 mL (0 °C)
44 g/100 mL (20 °C)
Solubility: insoluble in ethanol soluble in glycerol, water, and hydrogen iodide
Magnetic susceptibility (χ): −52.0·10−6 cm3/mol
Refractive index (nD):
1.468 (anhydrous)
1.394 (decahydrate)
Density: 2.70 g/cm3 (20 °C)
Melting Point: 888 °C
pH value: 5.2 - 8.0 (50 g/l, H₂O, 20 °C)
Bulk density: 1400 - 1600 kg/m3
Solubility: 200 g/l
Molecular Weight: 142.04 g/mol
Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 4
Rotatable Bond Count: 0
Exact Mass: 141.93126821 g/mol
Monoisotopic Mass: 141.93126821 g/mol
Topological Polar Surface Area: 88.6Ų
Heavy Atom Count: 7
Complexity: 62.2
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 3
Compound Is Canonicalized: Yes
Specifications of Sodium Sulfate:
Assay (alkalimetric): ≥ 99.0 %
Assay (alkalimetric, calculated on dried substance): 98.5 - 101.0 %
Identity: passes test
Appearance of solution: passes test
Insoluble matter: ≤ 0.01 %
Acidity or alkalinity: passes test
pH-value (5 %; water; 25 °C): 5.2 - 8.0
Chloride (Cl): ≤ 0.001 %
Phosphate (PO₄): ≤ 0.001 %
Total nitrogen (N): ≤ 0.0005 %
Heavy metals (ACS): ≤ 0.0005 %
Heavy metals (as Pb): ≤ 0.0005 %
As (Arsenic): ≤ 0.0001 %
Ca (Calcium): ≤ 0.005 %
Fe (Iron): ≤ 0.0005 %
K (Potassium): ≤ 0.002 %
Mg (Magnesium): ≤ 0.001 %
Loss on drying (130 °C): ≤ 0.5 %
Loss on ignition (800 °C): ≤ 0.5 %
Melting Point: 884°C
Quantity: 1000 g
Linear Formula: Na2SO4
Merck Index: 14,8680
Solubility Information: Soluble in water,glycerol and hydrogen iodide. Insoluble in ethanol and many organic solvents.
IUPAC Name: disodium;sulfate
Formula Weight: 142.04
Percent Purity: 99%
Odor: Odorless
Refractive Index: 1.484
Sensitivity: Hygroscopic
Density: 2.68
Chemical Name or Material: Sodium sulfate, anhydrous
Structure of Sodium Sulfate:
Crystal structure:
orthorhombic (anhydrous)
monoclinic (decahydrate)
Related compounds of Sodium Sulfate:
Sodium bisulfate
Sodium sulfite
Sodium persulfate
Other anions:
Sodium selenate
Sodium tellurate
Other cations:
Lithium sulfate
Potassium sulfate
Rubidium sulfate
Caesium sulfate
Names of Sodium Sulfate:
IUPAC name:
Sodium sulfate
Other names:
Sodium sulphate
Disodium sulfate
Sulfate of sodium
Thenardite (anhydrous mineral)
Glauber's salt (decahydrate)
Sal mirabilis (decahydrate)
Mirabilite (decahydrate mineral)
Synonyms of Sodium Sulfate:
SODIUM SULFATE
7757-82-6
Disodium sulfate
Sodium sulfate, anhydrous
Sodium sulfate anhydrous
Salt cake
Sodium sulphate
sodiumsulfate
Sulfuric acid disodium salt
Disodium sulphate
Sulfuric acid, sodium salt
15124-09-1
disodium;sulfate
Sulfate, sodium
Sodium sulphate anhydrous
Sodium sulfate, dried [JAN]
Sodium sulfate, dried
Na2SO4
MFCD00003504
Sodium sulphate, anhydrous
DTXSID1021291
CHEBI:32149
36KCS0R750
NSC-403914
13759-07-4
Sodium sulfate, dried (JAN)
Dibasic sodium sulfate
Natriumsulfat (German)
Na sulphate
Caswell No. 793
HSDB 5042
Sulfuric acid sodium salt (1:2)
Na2O4S
Thenardite (Na2(SO4))
Natriumsulfat
UNII-36KCS0R750
EINECS 231-820-9
EINECS 268-366-6
EINECS 268-773-9
EINECS 270-211-2
EPA Pesticide Chemical Code 005604
NSC 403914
Sodium sulfate anyhdrous
Sodium Sulfate ACS HE
AI3-02398
SDA 17-062-04
Sulfuric acid sodium salt
EC 231-820-9
SODIUM SULFATE [MI]
Sodium sulfate, ACS reagent
Sodium sulfate, dried (TN)
SODIUM SULFATE [HSDB]
CHEMBL233406
DTXCID601291
Anhydous sodium sulfate (JP17)
Sodium Sulfate - Drilling Grade
BCP13313
Tox21_201045
SODIUM SULFATE ANHYDROUS [II]
AKOS015833463
ANHYDROUS SODIUM SULFATE [JAN]
Sodium Sulfate Anhydrous Granular ACS
Sodium sulfate, BioXtra, >=99.0%
Sulfuric acid disodium salt, anhydrous
DB09472
ANHYDROUS SODIUM SULFATE [MART.]
NCGC00258598-01
Sodium sulfate, LR, anhydrous, >=99%
E514
SODIUM SULFATE ANHYDROUS [USP-RS]
SODIUM SULFATE ANHYDROUS [WHO-DD]
Sodium Sulfate Anhydrous; Sodium sulphate
CAS-7757-82-6
SODIUM SULFATE, ANHYDROUS [WHO-IP]
Sodium sulfate, AR, anhydrous, >=99.5%
FT-0645112
S0566
Sodium sulfate, 99.9955% (metals basis)
Sodium sulfate, ReagentPlus(R), >=99.0%
SODIUM SULFATE ANHYDROUS [ORANGE BOOK]
Sodium sulfate, Trace metals grade, 99.99%
D01732
NATRII SULFAS ANHYDRICUS [WHO-IP LATIN]
Sodium sulfate, >=99.99% trace metals basis
Sodium sulfate, JIS special grade, >=99.0%
Sodium sulfate, Vetec(TM) reagent grade, 99%
SODIUM SULFATE ANHYDROUS [USP MONOGRAPH]
SODIUM SULFATE, ANHYDROUS [EP MONOGRAPH]
Sodium sulfate, meets USP testing specifications
Q211737
Sodium sulfate, for HPLC, 99.0-101.0% (T)
Sodium sulfate, purum, anhydrous, >=99.0% (T)
Sodium sulfate, SAJ first grade, >=99.0%, beads
Sodium sulfate, SAJ first grade, >=99.0%, powder
Sodium sulfate, >=99.0%, plant cell culture tested
Sodium sulfate, BioUltra, anhydrous, >=99.0% (T)
Sodium sulfate, p.a., 99.0-101.0%, reag. ISO
Sodium sulfate, tested according to Ph.Eur., anhydrous
SULFURIC ACID DISODIUM SALT, ANHYDROUS [WHO-IP]
Sodium sulfate, ACS reagent, >=99.0%, anhydrous, powder
Sodium sulfate, ACS reagent, >=99.0%, anhydrous, granular
Sodium sulfate, anhydrous, free-flowing, Redi-Dri(TM), ACS reagent, >=99%
Sodium sulfate anhydrous, United States Pharmacopeia (USP) Reference Standard
Sodium sulfate, anhydrous, free-flowing, Redi-Dri(TM), ReagentPlus(R), >=99%
Sodium sulfate, anhydrous, granular, free-flowing, Redi-Dri(TM), ACS reagent, >=99%
Sodium sulfate, puriss. p.a., ACS reagent, reag. ISO, reag. Ph. Eur., anhydrous, >=99.0%
Sodium sulfate [Wiki]
231-820-9 [EINECS]
7757-82-6 [RN]
Bisodium sulfate
Dibasic sodium sulfate
Dinatriumsulfat [German] [ACD/IUPAC Name]
Disodium monosulfate
Disodium sulfate [ACD/IUPAC Name]
disodium sulphate
MFCD00003504 [MDL number]
Na2SO4 [Formula]
Natrii sulfas anhydricus
Natriumsulfat
sodium sulphate
Sulfate de disodium [French] [ACD/IUPAC Name]
Sulfate, sodium
Sulfuric acid disodium salt
Sulfuric acid, disodium salt
thenardite [Wiki]
231-550-1 [EINECS]
231-665-7 [EINECS]
268-366-6 [EINECS]
268-773-9 [EINECS]
270-211-2 [EINECS]
7757-82-6 (anhyd.)
Anhydrous sodium sulfate
disodium and sulfate
disodium;sulfate
Glauber's salt
Glaubers Salt
GoLYTELY
kemol
Kemsol
MFCD00149189 [MDL number]
natrium sulfate
Natriumsulfat (German)
SODIUM SULFATE (2:1) [ACD/IUPAC Name]
Sodium sulfate anyhdrous
Sodium sulfate, ACS reagent
Sodium sulfate,anhydrous
Sodium Sulphate Anhydrous
Sodium sulphate, anhydrous
Sodiumsulfate
Sulfuric acid disodium salt, anhydrous
Sulfuric acid sodium salt
SULFURIC ACID SODIUM SALT (1:2)
Sulfuric acid, sodium salt
