Description
Sodium Sulfate(7757-82-6), Na2S04, also known as thenardite and salt cake, is a crystalline compound that melts at 888°C (1632°F). Sodium Sulfate is found in natural form(thenardite) in Chile and Spain. It 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. It is used in dyeing,manufacturing glass,and in the preparation of sodium bisulfate.
sodium sulfate powder
Chemical raw materials
Sodium sulfate(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. It can also be used as filler of synthetic detergent. In the paper industry, it 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 ℃. It can be dissolved in water with the aqueous solution being neutral. It is soluble in glycerol and insoluble in ethanol. It is easy to absorb water when being exposed to become hydrous sodium sulfate. It is a homogeneous polycrystalline material and is rhombus at a temperature of 32.4~223 ℃ with generating shaped monoclinic crystal at higher temperatures and generating hexagonal crystals in 241 ℃. When being crystallized from solution, it 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 ℃. Another is sodium sulfate decahydrate Na2SO4·10H2O with conventional name being Glauber's salt, “YuanMingFen”, insurance powder. It appears as colorless monoclinic crystal with the density being 1.464g/cm3, the melting point of 32.38 ℃ and loss of crystal water to becomes anhydrous sodium sulfate at 100 ℃. It 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 it as mordant agent for making sodium sulfide, glass, water glass, enamel, quantitative measurement of nitrogen and papermaking pulp. In medical care field, it 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. Sulfate decahydrate, when being heated to the melting point (32.38 ℃), it 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 sulfate is being prone to become supersaturated solution.
The main function
Sodium sulfate 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 sulfate is the component of synthetic detergent and is a neutral salt. It can be added to the detergent to reduce the surface tension as well as increases the solubility of the detergent. It 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, it can be used as the raw material for the manufacturing of sodium sulfide, gypsum, sodium silicate and other chemical products. It 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, it has not yet been widely applied. It 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. It can increase the volume of the intestines and induce intestinal peristalsis with diarrhea effect. Sodium sulfate 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.
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 it 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. It is clinically mainly used in the treatment of large intestine constipation, eliminating the intestinal toxins as well as getting rid of parasites.
Solubility in water (g / 100ml)
The amount (grams) can be dissolved per 100 ml of water at different temperatures (℃):
4.9g/0 ℃; 9.1g/10 ℃; 19.5g/20 ℃; 40.8g/30 ℃; 48.8g/40 ℃
45.3g/60 ℃; 43.7g/80 ℃; 42.7g/90 ℃; 42.5g/100 ℃
Identification test
Sodium test of 5% of the sample liquid (IT-28) and sulfate test (IT-29) result is positive.
Content Analysis
Accurately weigh 500 mg of sample pre-dried for 4 h at 105 ℃ and dissolve it 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 it with the mass of barium sulphate then multiplying by 0.6086, namely is equivalent to sodium sulfate (of Na2SO3) content.
Toxicity
ADI does not make restrictive regulations (FAO/WHO, 2001).
GRAS (FDA, §186. 1797, 2000).
LD50: 5989mg/kg (mice through oral administration).
Chemical Properties
It appears as white monoclinic crystal or powder. It can be dissolved in water with the aqueous solution being alkaline. IT can be dissolved in glycerol and is insoluble in ethanol.
Uses
It can be mainly used as the filler of synthetic detergent. Paper industry applies it for the cooking agent during the manufacture of sulfate pulp. Glass industry uses it as substitute of soda. Chemical industry applies it as the raw material for the manufacturing of sodium sulfide, sodium silicate and other chemical products. Textile industry applies it for the formulation of Vinylon spinning coagulation bath. The pharmaceutical industry applies it as laxatives. It can also be used in non-ferrous metallurgy and leather.
Production method
Vacuum evaporation method: clarify the natural Glauber's salt after dissolving it; put the clarified solution for vacuum evaporation dehydration, thickening, centrifugation and separation and drying to obtain anhydrous sodium sulfate. The reaction equation is:
Na2SO4·10H2O → Na2SO4 + 10H2O
Calcium mirabilite method: crush the ore of calcium mirabilite, add water ball for grinding, leach, with the leached Glauber's salt being subject to removal of impurities via filtering out. After the clarification of the filtrate, then perform evaporation for dehydration, centrifugation, drying to obtain the anhydrous sodium sulfate. The reaction is:
Na2SO4·CaSO4 + 2H2O → Na2SO4 + CaSO4·2H2O
Conversion method uses the byproduct, high and low-temperature salt produced from potassium chloride as the raw material for making anhydrous sodium sulfate. Under certain conditions of temperature and ingredients, through three sections of transformation, magnesium sulfate and sodium chloride have been first converted into bloedite and then further converted to anhydrous sodium magnesium sulfate and finally being converted to anhydrous sodium sulfate. The entire conversion process is a continuous countercurrent operation with pulp relying the mechanical driving and elevation, liquid undergoing reverse overflow via potential difference. The conversion of the first segment is controlled at Ph value of 3 to 4 with reaction at a temperature of 55~70 ℃. The generated white sodium magnesium alumina slurry, after entering into a settler for thickening and then sent to the secondary conversion tank; secondary conversion has Ph of 4~5 and temperature of about 100 ℃; third conversion conditions is controlled at Ph5~6 with the temperature being about 55 ℃. Under stirring, the anhydrous loeweite can react with an aqueous solution of sodium chloride to generate anhydrous sodium sulfate crude product with centrifuge, separation, drying to obtain the anhydrous sodium sulfate to obtain. The reaction equation is:
2NaCl + 2MgSO4 + 4H2O → Na2SO4·MgSO4·4H2O + MgC12
Na2SO4·MgSO4·4H20 → Na2SO4·MgSO4 + 4H2O
Na2SO4·MgSO4 + 2NaCl → 2Na2SO4 + MgCl2
This method has high cost, low recycling rate with sulfuric acid consumption and the impurities not being prone to be removed. The resulting product is of poor color, but with simple equipment.
Rayon byproduct method: the rayon solidification waste undergoes crystallization, dissolution, neutralization, filtration, concentration, cooling, separation and drying process to obtain anhydrous sodium sulfate. The reaction equation is:
H2SO4 + 2NaOH → Na2SO4 + 2H2O
Chemical Properties
Sodium sulfate, NaS04, 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. The hydrate, Na2S04·10H20, also known as "Glauber's salt," is a white water-soluble solid formed by heating sodium chloride and sulfuric acid. It is used in dyeing,manufacturing glass,and in the preparation of sodium bisulfate.
Chemical Properties
Sodium sulfate is a white crystalline solid. It frequently is found as the decahydrate
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/cm
3; 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/cm
3; 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 Na
2SO
4, mirabilite is a naturallyoccurring decahydrate, Na
2SO
4?10H
2O.
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.
Sodium sulfate is used in manufacturing paper pulp by the Kraft Process. Other uses are in manufacturing glass and ultramarine; in dyeing and printing textiles; as a filler in synthetic detergents; and for standardizing dyes. A major use of anhydrous sodium sulfate is as an agent to remove water from organic solvents and their extracts for organic synthesis and instrumental analysis. Sodium sulfate is a common laboratory reagent. Also, it is used to prepare other sodium salts.
Uses
Sodium sulfate is a filler in the manufacturing of synthetic detergents and soaps and a laboratory reagent. It may enhance the irritant action of certain detergents.
Uses
Used in kjeldahl nitrogen determination; drying agent .
Uses
Sodium Sulfate is the salt of sulfuric acid that is readily soluble in
water and exists as crystals or crystalline powder. it is used in cara-
mel production.
Production Methods
Sodium sulfate is mined from its natural mineral deposits and subjected to purification.
Sodium sulfate 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 + H
2SO
4 → Na
2SO
4 + 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. It is a variation of Mannheim’s method. In this method, sulfur dioxide is used instead of sulfuric acid. The reaction is as follows: 4NaCl + 2SO
2 + O
2 + 2H
2O → 2Na
2SO
4 + 4HCl↑
Sodium sulfate also is obtained as a byproduct of manufacturing phenol by caustic fusion.
Definition
A white crystalline compound, Na
2SO
4, usually known as the anhydrous compound (orthorhombic; r.d. 2.67; m.p. 888°C) or the decahydrate (monoclinic; r.d. 1.46; which loses water at 100°C). The decahydrate is known as Glauber’s salt. A metastable heptahydrate (Na
2SO
4·7H
2O) also exists. All forms are soluble in water, dissolving to give a neutral solution. The compound occurs naturally as
mirabilite (Na
2SO
4·10H
2O),
threnardite (Na
2SO
4), and
glauberite (Na
2SO
4·CaSO
4).
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. It also finds medicinal application as a purgative and in commercial aperient salts.
General Description
Sodium sulfate (Na
2SO
4) can be obtained directly via precipitation from a saturated solution of Na
2SO
4 at room temperature (20°C). Its crystallization and growth rates at room temperature (20°C) under various conditions have been investigated. Sodium sulfate can be produced during Leblanc process, from sodium chloride and sulfuric acid.
Flammability and Explosibility
Non flammable
Safety Profile
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. See also SULFATES.
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.
Veterinary Drugs and Treatments
Sodium sulfate 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. It 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.
