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Sodium sulphates (also known as sodium 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.
With an annual production of 6 million tonnes, the decahydrate is a major commodity chemical product.
Sodium sulhates 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.
CAS: 7757-82-6
MF: Na2SO4
MW: 142.04214
EINECS: 231-820-9
Synonyms:
Bisodium sulfate;bisodiumsulfate;Crimidesa;Crude sodium sulfate;dibasicsodiumsulfate;Disodium monosulfate;Disodium sulphate;disodiummonosulfate
Melting point: 884 C (lit.)
Boiling point: 1700C
density: 2.68 g/mL at 25 C (lit.)
bulk density: 1400-1600kg/m3
refractive index : 1.484
storage temp.: Store at +5C to +30C.
solubility: H2O: 1 M at 20 C, clear, colorless
form: powder (fine)
pka: 4.76
Specific Gravity: 2.68
color : White
PH: 5.2-8.0 (50g/l, H2O, 20C)
PH Range: 5.2 - 9.2
Odor: wh.
cryst. or powd., odorless, bitter saline taste
Water Solubility : 18.5 mg/L
Sensitive: Hygroscopic
lmax: l: 260 nm Amax: 0.015
l: 280 nm Amax: 0.015
Merck : 14,8680
Dielectric constant: 2.7 (Ambient)
Stability: Stable.
Incompatible with strong acids, aluminium, magnesium, strong bases. Hygroscopic.
Cosmetics Ingredients Functions: BULKING
VISCOSITY CONTROLLING
InChI: 1S/2Na.H2O4S/c;;1-5(2,3)4/h;;(H2,1,2,3,4)/q2+1;/p-2
InChIKey: PMZURENOXWZQFD-UHFFFAOYSA-L
LogP: -1.031 (est)
CAS DataBase Reference: 7757-82-6(CAS DataBase Reference)
NIST Chemistry Reference: Sodium sulfate(7757-82-6)
EPA Substance Registry System: Sodium sulfate (7757-82-6)
Forms
Anhydrous Sodium sulphates, 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 sulhates is also known as Glauber's salt.
History
The decahydrate of Sodium sulphates is known as Glauber's salt after the Dutch-German chemist and apothecary Johann Rudolf Glauber (1604-1670), who discovered Sodium sulhates in Austrian spring water in 1625.
He named Sodium sulphate sal mirabilis (miraculous salt), because of its medicinal properties: the crystals were used as a general-purpose laxative, until more sophisticated alternatives came about in the 1900s.
However, J. Kunckel later alleged that Sodium sulphate was known as a secret medicine in Saxony already in the mid-16th century.
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.
Description
Sodium sulphates(7757-82-6), Na2S04, also known as thenardite and salt cake, is a crystalline compound that melts at 888C (1632F).
Sodium sulphates is found in natural form(thenardite) in Chile and Spain.
Sodium sulphates is used in the manufacture of paperboard, glass,and freezing mixtures.
The hydrate, Na2S04.10H20, also known as "Glauber's salt," is a white water-soluble solid formed by heating Sodium chloride and sulfuric acid.
Sodium sulphates is used in dyeing,manufacturing glass,and in the preparation of sodium bisulfate.
General Description
Sodium sulphates (Na2SO4) can be obtained directly via precipitation from a saturated solution of Na2SO4 at room temperature (20C).
Its crystallization and growth rates at room temperature (20C) under various conditions have been investigated.
Sodium sulphates can be produced during Leblanc process, from sodium chloride and sulfuric acid.
Chemical raw materials
Sodium sulphates(7757-82-6) is an important chemical raw material and is the main raw material for production of sodium sulfide, sodium silicate and other chemical products.
Sodium sulphate can also be used as filler of synthetic detergent.
In the paper industry, Sodium sulphate can be used as the cooking agent for the manufacturing of paper pulp of sulfate.
Sodium sulfate, also known as anhydrous Glauber's salt or anhydrous mirabilite, appears as white monoclinic crystal or fine powder with the relative density being 2.68 and the melting point being 884 C.
Sodium sulphates can be dissolved in water with the aqueous solution being neutral.
Sodium sulphates is soluble in glycerol and inaccessible in ethanol.
Sodium sulphates is easy to absorb water when being exposed to become hydrous sodium sulfate.
Sodium sulphates is a homogeneous polycrystalline material and is rhombus at a temperature of 32.4~223 C with generating shaped monoclinic crystal at higher temperatures and generating hexagonal crystals in 241 C.
When being crystallized from solution, Sodium sulphate has high affinity to iron, iron compound and various kinds of other organic compounds;
high-purity, fine-particle anhydrous sodium sulfate is called as YuanMingFen.
There are two kinds of crystalline hydrate compound of sodium sulfate: one is heptahydrate sodium Na2SO4.7H2O, being white sixty or tetragonal crystal with dehydrating at 24.4 C.
Another is sodium sulfate decahydrate Na2SO4.10H2O with conventional name being Glauber's salt, YuanMingFen, insurance powder.
Sodium sulphates appears as colorless monoclinic crystal with the density being 1.464g/cm3, the melting point of 32.38 C and loss of crystal water to becomes anhydrous Sodium sulphates at 100C.
Sodium sulphates is easily soluble in water and is easily weathered in dry air to become a dry white powder.
Sodium sulfate can be used as chemical analysis reagent such as dye testing;
printing industry apply Sodium sulphate as mordant agent for making sodium sulfide, glass, water glass, enamel, quantitative measurement of nitrogen and papermaking pulp.
In medical care field, Sodium sulphate can be used as the antidotes of medical diuretics, laxatives and barium salt poisoning.
There are also sodium salt crystals precipitated from salt ponds in winter.
Naturally occurring sulfate mineral is widely distributed with mostly existing in magnesium sulfate (calcium) complex salt and mirabilite.
There are relative large amount of salt lakes in China's Inner Mongolia, Qinghai, Tibet, and some places of Xinjiang.
There is large amount of sodium sulfate in the salt lake.
Industrial preparation of sodium sulfate is mainly isolated from natural mineral or by the mirabilite dehydration and treatment with sulfuric acid to obtain sodium chloride.
Sodium sulfate is also the byproduct of a lot of chemical industrial production sector and can be extracted from the waste liquid discharged during the production of viscose fiber and cellophane.
In the production of sodium dichromate, phenols, boric acid, lithium carbonate, and certain pigments, there is also sodium sulfate as byproduct.
Sodium sulphates decahydrate, when being heated to the melting point (32.38 C), Sodium sulphate can be dissolved its own crystal water while generating anhydrous salt.
This temperature is the temperature at which the decahydrate salt, anhydrous salt and saturated solution, the three-phases reaches equilibrium temperature.
As long as the three-phase coexists, the temperature is constant.
Therefore the system can be used for as constant temperature bath or for calibration of temperature.
Another feature of Sodium sulphates is being prone to become supersaturated solution.
Chemical properties
Sodium sulphates 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 sulphates is unreactive toward most oxidizing or reducing agents.
At high temperatures, Sodium sulphates can be converted to sodium sulfide by carbothermal reduction (aka thermo-chemical sulphates sulphates 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 sulphates reacts with sulfuric acid to give the acid salt sodium bisulfate:
Na2SO4 + H2SO4 -> 2 NaHSO4
Sodium sulphates 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 sulphate 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 sulphates 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.
The main function
Sodium sulphates is an important raw material in the manufacturing of glass and paper with the maximum usage amount in the paper and cellulose industry which accounts for around 70% of the total amount.
Sodium sulphates is the component of synthetic detergent and is a neutral salt.
Sodium sulphates can be added to the detergent to reduce the surface tension as well as increases the solubility of the detergent.
Sodium sulphates is also be used as the dye diluent and the auxiliary agent of the dye printing, as direct dyes, sulfur dyes, vat dyes and other accelerant of dyed cotton fiber, as retarding agent for direct dye silk.
In the chemical industry, Sodium sulphates can be used as the raw material for the manufacturing of sodium sulfide, gypsum, sodium silicate and other chemical products.
Sodium sulphates has been now developed of the method for making sulfuric acid, sulfur, soda ash, ammonium sulfate and other products with sodium sulfate.
However, due to the high cost of these methods, Sodium sulphate has not yet been widely applied.
Sodium sulphates has been commonly used by laboratory system for using sodium sulfate as cold agent.
Glauber's salt has been used as a laxative medicine.
The sodium sulfate entering into the body is largely stuck in the gastrointestinal tract without being absorbed and being maintained at certain penetration.
Sodium sulphates can increase the volume of the intestines and induce intestinal peristalisis with diarrhea effect.
Sodium sulphates is the antidote of barium and lead poisoning.
Upon lead poisoning, people can apply gastric lavage with 10% Glauber's salt or orally administer 1 to 2% sodium sulfate solution.
The above information is edited by the chemicalbook of Dai Xiongfeng.
Physical properties
Sodium sulphates has unusual solubility characteristics in water.
Sodium sulphates solubility in water rises more than tenfold between 0 C and 32.384 C, where Sodium sulphate 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.
Physical properties
Anhydrous sodium sulfate is a white crystalline powder; orthorhombic or hexagonal structure; hygroscopic; refractive index 1.468; hardness 2.8 Mohs;
density 2.664 g/cm3; melts at 884C; soluble in water, insoluble in ethanol.
The decahydrate consists of colorless monoclinic crystals;
refractive index 1.394; hardness 1.8 Mohs; density 1.46g/cm3; decomposes at 32C; soluble in water; insoluble in ethanol.
Potential Exposure
Sodium sulphates 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.
Veterinary Drugs and Treatments
Sodium sulphates is used as a saline cathartic, primarily in food animals.
Shipping
UN2630 Selenates or Selenites, Hazard Class: 6.1; Labels: 6.1-Poisonous materials.
Purification Methods
Crystallise sodium sulfate from water at 30o (1.1mL/g) by cooling to 0o. Sodium sulphate becomes anhydrous at 32o.
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.
Content Analysis
Accurately weigh 500 mg of sample pre-dried for 4 h at 105 C and dissolve Sodium sulphate in 200ml of water;
Add 1 mL of hydrochloric acid and heat to boiling.
Under constant stirring, add in portions of a small amount (around 10 mL) of hot barium chloride test solution (TS-37), heat on a steam bath for 1h and filter out the precipitate with further washing with water until being chloride-free.
After drying, burn and weigh Sodium sulphate with the mass of barium sulphate then multiplying by 0.6086, namely is equivalent to Sodium sulphate (of Na2SO3) content.
Toxicity
ADI does not make restrictive regulations (FAO/WHO, 2001).
GRAS (FDA, section 186. 1797, 2000).
LD50: 5989mg/kg (mice through oral administration).
Chemical Properties
Sodium sulphate appears as white monoclinic crystal or powder.
Sodium sulphate can be dissolved in water with the aqueous solution being alkaline.
Sodium sulphate can be dissolved in glycerol and is insoluble in ethanol.
Uses
Sodium sulphate can be mainly used as the filler of synthetic detergent.
Paper industry applies Sodium sulphate for the cooking agent during the manufacture of sulfate pulp.
Glass industry uses Sodium sulphate as substitute of soda.
Chemical industry applies Sodium sulphate as the raw material for the manufacturing of sodium sulfide, sodium silicate and other chemical products.
Textile industry applies Sodium sulphate for the formulation of Vinylon spinning coagulation bath.
The pharmaceutical industry applies Sodium sulphate as laxatives.
Sodium sulphate can also be used in non-ferrous metallurgy and leather.
Used in kjeldahl nitrogen determination; drying agent .
Sodium sulphates is a filler in the manufacturing of synthetic detergents and soaps and a laboratory reagent.
Sodium sulphate may enhance the irritant action of certain detergents.
Sodium sulphate is the salt of sulfuric acid that is readily soluble in water and exists as crystals or crystalline powder.
Sodium sulphate is used in caramel production.
Pharmacological effects
Apply oral administration of small amount with its ionic and osmotic pressure effect being able to slightly stimulate the digestive tract mucosa and causes a slight increase of the gastrointestinal secretion and a slight increase in the movement, therefore Sodium sulphate has stomachic effect.
Orally administer a large amount with a lot of sodium sulfate being dissolved in large amount of water for oral administration.
Since the ions are not easily absorbed and can maintain large amount of water in the intestines and can mechanically stimulate the intestinal mucosa and can soften the fecal matter and accelerate the defecation.
Sodium sulphates is clinically mainly used in the treatment of large intestine constipation, eliminating the intestinal toxins as well as getting rid of parasites.
Structure
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 its ability to distribute water much more rapidly compared to most hydrates.
Production
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), Quimica 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 (Dongpo District, Meishan, Sichuan, China), and Kuchuksulphat JSC (Altai Krai, Siberia, Russia).
Anhydrous sodium sulfate occurs in arid environments as the mineral thenardite.
Sodium sulphates slowly turns to mirabilite in damp air.
Sodium sulphates 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.[21]
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 historically 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.
2NaOH(aq) + H2SO4(aq) -> Na2SO4(aq) + 2 H2O(l) DH = -112.5 kJ (highly exothermic)
In the laboratory Sodium sulphate can also be synthesized from the reaction between sodium bicarbonate and magnesium sulfate,by precipitating magnesium carbonate.
2NaHCO3 + 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).
Production Methods
Sodium sulphates is mined from its natural mineral deposits and subjected to purification.
Sodium sulphates is synthesized by the Mannheim process or Hargreaves process.
Manheim's process is based on Glauber's reaction between sulfuric acid and sodium chloride: 2NaCl + H2SO4 -> Na2SO4 + 2HCl
The process was devised by Johann Glauber to produce hydrochloric acid.
Sodium sulfate is isolated from the solution by fractional crystallization.
Hargreaves' process also was developed to produce hydrochloric acid.
Sodium sulphate is a variation of Mannheim's method.
In this method, sulfur dioxide is used instead of sulfuric acid.
The reaction is as follows: 4NaCl + 2SO2 + O2 + 2H2O -> 2Na2SO4 + 4HCl
Sodium sulphates also is obtained as a byproduct of manufacturing phenol by caustic fusion.
Definition
A white crystalline compound, Na2SO4, usually known as the anhydrous compound (orthorhombic; r.d. 2.67; m.p. 888C) or the decahydrate (monoclinic; r.d. 1.46; which loses water at 100C).
The decahydrate is known as Glauber's salt.
A metastable heptahydrate (Na2SO4.7H2O) also exists.
All forms are soluble in water, dissolving to give a neutral solution.
The compound occurs naturally as
mirabilite (Na2SO4.10H2O),
threnardite (Na2SO4), and
glauberite (Na2SO4.CaSO4).
Sodium sulphate may be produced industrially by the reaction of magnesium sulphate with sodium chloride in solution followed by crystallization, or by the reaction of concentrated sulphuric acid with solid sodium chloride.
The latter method was used in the Leblanc process for the production of alkali and has given the name salt cake to impure industrial sodium sulphate.
Sodium sulphate is used in the manufacture of glass and soft glazes and in dyeing to promote an even finish.
Sodium sulphate also finds medicinal application as a purgative and in commercial aperient salts.
Applications
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 sulphate 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 sulphate.
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 sulphate is used as a fining agent, to help remove small air bubbles from molten glass.
sodium sulphate 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 sulphate is important in the manufacture of textiles, particularly in Japan, where Sodium sulphate is the largest application.
sodium sulphate 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 sulphate 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 sulphate 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 this material especially appropriate for storing low-grade solar heat for later release in space heating applications.
In some applications the material 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 the material 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 sulphate is more efficient, but slower-acting, than the similar agent magnesium sulfate.
Sodium sulphate is only effective below about 30 C (86 F), but sodium sulphate can be used with a variety of materials since sodium sulphate is chemically fairly inert.
sodium sulphate 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 sulphate is effective for the removal of certain drugs, such as paracetamol (acetaminophen) from the body;
thus Sodium sulphate can be used after an overdose.
In 1953, sodium sulfate was proposed for heat storage in passive solar heating systems.
This takes advantage of its unusual solubility properties, and the high heat of crystallisation (78.2 kJ/mol).
Other uses for sodium sulphate 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.
The material slowly turns to liquid and recirculates, equalizing laptop temperature and acting as an insulation.
Chemical Properties
Sodium sulfate is a white crystalline solid.
Sodium sulphate frequently is found as the decahydrate
Sodium sulfate, NaS04, also known as thenardite and salt cake, is a crystalline compound that melts at 888C (1632C).
Sodium sulfate is found in natural form(thenardite) in Chile and Spain.
Sodium sulphate is used in the manufacture of paperboard, glass,and freezing mixtures.
The hydrate, Na2S04.10H20, also known as "Glauber's salt," is a white water-soluble solid formed by heating sodium chloride and sulfuric acid.
Sodium sulphate is used in dyeing,manufacturing glass,and in the preparation of sodium bisulfate.
Safety
Although sodium sulfate is generally regarded as non-toxic,sodium sulphates 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.
Raw materials
Sodium nitrite->Sodium chloride->Dimethyl sulfate->Potassium chloride->Sodium formate->SODIUM SULFATE DECAHYDRATE->Paste->GLAUBERITE->bloedite
Preparation Products
Cilostazol->Creatine phosphate disodium salt->1-(5-BROMO-1-BENZOFURAN-2-YL)ETHANONE->1-(2-PHENOXYETHYL)-PIPERAZINE->7-HYDROXY-4-(TRIFLUOROMETHYL)COUMARIN->IODOCYCLOHEXANE->3-TERT-BUTYLISOXAZOL-5-AMINE->Acid Red 73->Direct Black 56->2,4-Dichloro-5-fluoronitrobenzene->DIOCTYL ETHER->N-Methyl-1-(pyridin-4-yl)methanamine->Dimethyl itaconate->2'-AMINOACETANILIDE-->Cerium dioxide->fluorescent whitening agent DMS->Sodium bisulfate monohydrate->Pravastatin->Acid Blue 93->pesticide emalsifier 2000->4-HYDROXY-6-MERCAPTOPYRAZOLO[3,4-D]PYRIMIDINE->DIRECT BLUE 15->IMIBENCONAZOLE->Early-strength admixture->Direct Blue 151->Direct Black 38->fluorescent whitening agent RA->sec-Pentanol->sopa->PROCION RED MX-5B->fluorescent bleaches R->ACID RED 1->GLAUBERITE->dacron oiling agent 73->Direct Black BH->Mandarin oil->Barium sulfate,superfine->Patent Blue VF->Trypan Blue->2-Chloro-4-methylsulphonylbenzoic acid
