SODIUM CARBONATE

SODIUM CARBONATE = SODA = SODA ASH = SODA CRYSTALS 

CAS Number: 497-19-8
EC Number: 207-838-8
MDL number: MFCD00003494
Molecular Formula: Na2CO3

Sodium carbonate, Na2CO3·10H2O, (also known as Natrium Carbonate, washing soda, soda ash and soda crystals) is the inorganic compound with the formula Na2CO3 and Sodium carbonate's various hydrates. 
All forms are white, odourless, water-soluble salts that yield moderately alkaline solutions in water. 
Historically, Sodium carbonate was extracted from the ashes of plants growing in sodium-rich soils. 
Because the ashes of these sodium-rich plants were noticeably different from ashes of wood (once used to produce potash), sodium carbonate became known as "soda ash". 

Sodium carbonate is produced in large quantities from sodium chloride and limestone by the Solvay process.
Sodium carbonate is soluble in water, and can occur naturally in arid regions, especially in mineral deposits (evaporites) formed when seasonal lakes evaporate. 
Deposits of the mineral natron have been mined from dry lake bottoms in Egypt since ancient times, when natron was used in the preparation of mummies and in the early manufacture of glass.
The anhydrous mineral form of sodium carbonate is quite rare and called natrite. 

Sodium carbonate also erupts from Ol Doinyo Lengai, Tanzania's unique volcano, and Sodium carbonate is presumed to have erupted from other volcanoes in the past, but due to these minerals' instability at the earth's surface, are likely to be eroded. 
All three mineralogical forms of sodium carbonate, as well as trona, trisodium hydrogendicarbonate dihydrate, are also known from ultra-alkaline pegmatitic rocks, that occur for example in the Kola Peninsula in Russia.
Extraterrestrially, known sodium carbonate is rare. 

Deposits have been identified as the source of bright spots on Ceres, interior material that has been brought to the surface. While there are carbonates on Mars, and these are expected to include sodium carbonate, deposits have yet to be confirmed, this absence is explained by some as being due to a global dominance of low pH in previously aqueous Martian soil.
Sodium Carbonate is the disodium salt of carbonic acid with alkalinizing property. 
When dissolved in water, sodium carbonate forms carbonic acid and sodium hydroxide. 
As a strong base, sodium hydroxide neutralizes gastric acid thereby acting as an antacid.

Sodium carbonate is an organic sodium salt and a carbonate salt.
Sodium carbonate, or soda ash, Na2CO3, is widely distributed in nature, occurring as constituents of mineral waters and as the solid minerals natron, trona, and thermonatrite. 
Large quantities of this alkaline salt are used in making glass, detergents, and cleansers. 
Sodium carbonate is an inorganic chemical compound. 
Sodium carbonate is what is commonly known as Soda ash. 

Soda ash is extracted from trona. 
Trona is a double salt containing sodium carbonate and sodium hydrogen carbonate formed as a result of the series of evaporation processes taking place at lakes.
Sodium carbonate often called washing soda or soda ash is the most important of all basic heavy chemicals. 
Sodium carbonate's great advantage over sodium hydroxide is that Sodium carbonate is no-corrosive and is, therefore, safer to handle.

Sodium carbonate is a diazonium salt of carbonic acid with chemical formula Na2CO3. 
Sodium carbonate is also known as Soda crystals, soda ash, washing soda. 
Sodium carbonate is water-soluble and when dissolved in water, Sodium carbonate forms carbonic acid and sodium hydroxide. 
In Sodium carbonate's pure form, Sodium carbonate is white powder and odourless. 
Sodium carbonate is a strong base and acts as an antacid.

Sodium carbonate can be produced by four processes.
“Solvay process, Labnac process, Dual-process, Electrolytic process”. 
Since Sodium carbonate is a weak acid Sodium carbonate is slightly soluble in ethanol and insoluble in alcohol. 
One of the important uses of Na2CO3 is as a water softener. 
pH is about 11.
Sodium carbonate can be noted that each molecule of sodium carbonate contains 2 sodium atoms, 3 oxygen atoms and one carbon atom. 

Each sodium cation holds a charge of +1 whereas the polyatomic carbonate anion holds a net charge of magnitude -2. 
Sodium carbonate is, therefore, a neutrally charged molecule.
Sodium carbonate (also known as washing soda or soda ash), Na2CO3, is a sodium salt of carbonic acid and is a fairly strong, non-volatile base. 
Sodium carbonate most commonly occurs as a crystaline heptahydrate which readily effloresces to form a white powder, the monohydrate. 
Sodium carbonate has a cooling alkaline taste, and can be extracted from the ashes of many plants. 

Sodium carbonate is produced artificially in large quantities from common salt.
Sodium carbonate is either found naturally or is manufactured from sodium chloride (common salt). 
Sodium carbonate has many uses, notably to make glass. 
Two forms of sodium carbonate (soda ash) are used -heavy and light.  
The light form is obtained first and some is then converted into the heavy form.  
Light sodium carbonate contains less than 0.5% sodium chloride. 

Heavy sodium carbonate is obtained by hydrating light sodium carbonate to the monohydrate (Na2CO3.H2O) and then dehydrating Sodium carbonate to give a product with an increased crystal size and density.
The two grades have different uses.
The major uses of heavy sodium carbonate are as a solid, particularly in making glass, where Sodium carbonate is used as a flux in the melting of silica (sand).
The uses for light sodium carbonate are traditionally where the chemical is required in solution.

Sodium carbonate is an organic sodium salt and a carbonate salt. 
Sodium Carbonate is the disodium salt of carbonic acid with alkalinizing property. 
When dissolved in water, sodium carbonate forms carbonic acid and sodium hydroxide.
Sodium carbonate, Na2CO3, (also known as washing soda, soda ash and soda crystals, and in the monohydrate form as crystal carbonate) is the water-soluble sodium salt of carbonic acid.
Sodium carbonate most commonly occurs as a crystalline decahydrate, which readily effloresces to form a white powder, the monohydrate. 

Pure sodium carbonate is a white, odorless powder that is hygroscopic (absorbs moisture from the air). 
Sodium carbonate has a strongly alkaline taste, and forms a moderately basic solution in water. 
Sodium carbonate is well known domestically for Sodium carbonate's everyday use as a water softener. 
Historically Sodium carbonate was extracted from the ashes of plants growing in sodium-rich soils, such as vegetation from the Middle East, kelp from Scotland and seaweed from Spain. 
Because the ashes of these sodium-rich plants were noticeably different from ashes of timber (used to create potash), they became known as "soda ash". 

Sodium carbonate is synthetically produced in large quantities from salt (sodium chloride) and limestone by a method known as the Solvay process.
Sodium carbonate (Na2CO3) is the sodium salt of carbonic acid. 
Sodium carbonate is also known as sal soda, washing soda, soda ash and soda crystals. 
Sodium carbonate exists as a white powder, absorbs moisture from the air, and forms a strong alkaline aqueous solution. 
Sodium carbonate is commonly used as a water softener and is used to make glass. 
Sodium carbonate can exist in nature from the ashes of certain plants, and also can be derived synthetically in the lab from sodium chloride (salt) and limestone via the well-known Solvay process. 

Sodium carbonate is an odorless white powder or crystalline solid with an alkaline taste. 
Sodium carbonate is hygroscopic, meaning that it has a tendency to absorb moisture from the air. 
Sodium carbonate also exists as the monohydrate (Na2CO3·H2O) and as the decahydrate (Na2CO3·10H2O), each with slightly different physical properties from those of the anhydrous salt. 
The anhydrous form of sodium carbonate is commonly known as soda ash, while the decahydrate is often called sal soda or washing soda. 
Sodium carbonate has long been one of the most important chemical compounds produced in the United States. 
Sodium carbonate's primary use is in the manufacture of glass and other chemicals.

Sodium carbonate occurs naturally on earth, but may also be manufactured by mixing sodium chloride (salt) with ammonia. 
Pick up sodium carbonate at grocery stores or at swimming pool supply stores as well as hardware stores. 
The grey-white powder or solid white powder is odorless and tasteless.
Sodium carbonate is a white colored inorganic compound made up of sodium, carbon and oxygen elements. 
Sodium carbonate has various hydrated forms. 
Sodium carbonate has a strong alkaline taste. 

Sodium carbonate, also known as disodium carbonate or soda ash, is a member of the chlor-alkali chemical family and competes with caustic soda as a source of alkali (sodium oxide) in many processes. 
Commercial soda ash is highly purified and is sold in various grades that differ primarily in bulk density. 
Sodium carbonate is produced synthetically and from natural resources (primarily trona). 
Sodium carbonate is an inorganic compound containing a sodium salt of carbonic acid and has an alkaline taste. 
Sodium carbonate's chemical formula is Na2CO3.

Sodium carbonate is a white crystalline or powdered chemical that is odorless with an alkaline taste. 
Sodium carbonate comes from the ashes of plants that grow in sodium-rich soil. 
Also known as soda ash, sodium carbonate is sometimes produced synthetically from salt and limestone.
Soda ash, also known as sodium carbonate (Na2CO3), is an alkali chemical refined from the mineral trona or naturally occurring sodium carbonate-bearing brines (both referred to as natural soda ash), the mineral nahcolite (referred to as natural sodium bicarbonate, from which soda ash can be produced), or manufactured from one of several chemical processes (referred to as synthetic soda ash).
A series of refining steps are required to produce soda ash from trona ore. 

First the raw ore from the mine is crushed and screened. 
The materia l is then fed to rotary calciners and heated. 
In this process, the trona decomposes to form crude soda ash, which is dissolved in water. 
The insoluble shales are separated from the solution by a combination of settling and filtration steps, and the resulting insoluble tailings are taken back into the mine as backfill. 
The soda ash solution is treated to remove organic materials yielding a high-purity saturated solution of sodium carbonate.
Next, the solution is fed to crystallizers where water is evaporated and sodium carbonate monohydrate crystals are formed. 

The industry-familiar term "mono-process" originates from this process step. 
The crystals are dewatered and washed using cyclones and centrifuges, and the solution is recycled to the evaporator units for further recovery of soda ash. 
The monohydrate crystals are fed to rotary kilns where they are dried to finished soda ash. 
Finally, product is screened and sent to storage silos awaiting rail and truck loadout.
Sodium carbonate, chemical compound, Na2CO3, soluble in water and very slightly soluble in alcohol. 

Pure sodium carbonate is a white, odorless powder that absorbs moisture from the air, has an alkaline taste, and forms a strongly alkaline water solution. 
Sodium carbonate is one of the most basic industrial chemicals. 
Sodium carbonate decahydrate, Na2CO3·10H2O, is a colorless, transparent crystalline compound commonly called sal soda or washing soda. Because seaweed ashes were an early source of sodium carbonate, Sodium carbonate is often called soda ash or, simply, soda. 
Sodium carbonate’s common name is Washing soda and soda ash. 

Also, Sodium carbonate occurs naturally in arid (dry) regions of the earth.
Besides, find them in places where the lake have evaporated and we find them there in the form of deposits.  
In addition, Sodium carbonate is one of the most common industrial chemicals.
The formula of sodium carbonate happens to be  Na2CO3. 
In addition, all Sodium carbonate's forms are water-soluble salts and white in colour. 
Furthermore, all Sodium carbonate's form has an alkaline taste also in the water they are moderately alkaline.
If Sodium carbonate was extracted from the ashes of plants that grow in sodium-rich soils. 

Furthermore, these ashes are far different from ashes of wood and that’s why Sodium carbonate is called soda ash.
Sodium carbonate, commonly known as soda ash in Sodium carbonate's anhydrous form, is the sodium salt of carbonic acid with the chemical formula Na2CO3.  
Sodium carbonate occurs naturally in arid regions and is often extracted from mineral deposits of trona ore.  
Wyoming is the largest domestic source, with large natural trona deposits being mined.  
Sodium carbonate can occur naturally in the ashes of certain plants, and Sodium carbonate can also be derived synthetically from sodium chloride and limestone via the well-known Solvay process.  

Sodium carbonate is a stable, non-toxic odorless white powder that absorbs moisture and forms a strong alkaline aqueous 
solution.  
Sodium carbonate monohydrate (Na2CO3 H2O) has an added molecule of water and is often used as a buffer. 
Sodium carbonate (also known as washing soda or soda ash), Na2CO3, is a sodium salt of carbonic acid. 
Sodium carbonate most commonly occurs as a crystalline heptahydrate which readily effloresces to form a white powder, the monohydrate. 
Sodium carbonate has a cooling alkaline taste, and can be extracted from the ashes of many plants. 
Sodium carbonate is synthetically produced in large quantities from table salt in a process known as the Solvay process.

Sodium carbonate is soluble in water, but can occur naturally in arid regions, especially in the mineral deposits (evaporites) formed when seasonal lakes evaporate. 
Deposits of the mineral natron, a combination of sodium carbonate and sodium bicarbonate, have been mined from dry lake bottoms in Egypt since ancient times, when natron was used in the preparation of mummies and in the early manufacture of glass. 
Sodium carbonate has three known forms of hydrates: sodium carbonate decahydrate, sodium carbonate heptahydrate and sodium carbonate monohydrate.

USES and APPLICATIONS of SODIUM CARBONATE:
-Sodium carbonate (or washing soda) is used as a cleansing agent for domestic purposes like washing clothes. 
-Sodium carbonate is a component of many dry soap powders.
-It is used for removing temporary and permanent hardness of water.
-It is used in the manufacture of glass, soap and paper.
-It is used in the manufacture of sodium compounds like borax.

-Hard water contains dissolved compounds, usually calcium or magnesium compounds. 
Sodium carbonate is used for removing temporary and permanent hardness of water.
As sodium carbonate is water-soluble and magnesium carbonate and calcium carbonate are insoluble, the former is used to soften water by removing Mg2+ and Ca2+. 
These ions form insoluble solid precipitates upon treatment with carbonate ions.
The water is softened because it no longer contains dissolved calcium ions and magnesium ions.

-Sodium carbonate is used in the production of sherbet powder. 
The cooling and fizzing sensation results from the endothermic reaction between sodium carbonate and a weak acid, commonly citric acid, releasing carbon dioxide gas, which occurs when the sherbet is moistened by saliva.
-Sodium carbonate also finds use in the food industry as a food additive (E500) as an acidity regulator, anticaking agent, raising agent, and stabilizer.
Sodium carbonate is also used in the production of snus to stabilize the pH of the final product.

-Sodium carbonate is also used as a relatively strong base in various fields. 
As a common alkali, Sodium carbonate is preferred in many chemical processes because Sodium carbonate is cheaper than sodium hydroxide and far safer to handle. 
Sodium carbonate's mildness especially recommends Sodium carbonate's use in domestic applications.
-Sodium carbonate is used as a pH regulator to maintain stable alkaline conditions necessary for the action of the majority of photographic film developing agents. 

-Sodium carbonate is also a common additive in swimming pools and aquarium water to maintain a desired pH and carbonate hardness (KH). 
-In dyeing with fiber-reactive dyes, sodium carbonate (often under a name such as soda ash fixative or soda ash activator) is used to ensure proper chemical bonding of the dye with cellulose (plant) fibers, typically before dyeing (for tie-dyes), mixed with the dye (for dye painting), or after dyeing (for immersion dyeing). 
-Sodium carbonate is also used in the froth flotation process to maintain a favourable pH as a float conditioner besides CaO and other mildly basic compounds.

-Sodium bicarbonate (NaHCO3) or baking soda, also a component in fire extinguishers, is often generated from sodium carbonate. 
Although NaHCO3 is itself an intermediate product of the Solvay process, the heating needed to remove the ammonia that contaminates it decomposes some NaHCO3, making it more economic to react finished Na2CO3 with CO2.
In a related reaction, sodium carbonate is used to make sodium bisulfite (NaHSO3), which is used for the "sulfite" method of separating lignin from cellulose. 
This reaction is exploited for removing sulfur dioxide from flue gases in power stations.
This application has become more common, especially where stations have to meet stringent emission controls.

-Sodium carbonate is used by the cotton industry to neutralize the sulfuric acid needed for acid delinting of fuzzy cottonseed.
-Sodium carbonate is used by the brick industry as a wetting agent to reduce the amount of water needed to extrude the clay. -In casting, Sodium carbonate is referred to as "bonding agent" and is used to allow wet alginate to adhere to gelled alginate. 
-Sodium carbonate is used in toothpastes, where Sodium carbonate acts as a foaming agent and an abrasive, and to temporarily increase mouth pH.

-Sodium carbonate is also used in the processing and tanning of animal hides.
-Alkalizing buffering action: 
Sodium bicarbonate is an alkalinizing agent that dissociates to provide bicarbonate ion. Bicarbonate in excess of that needed to buffer hydrogen ions causes systemic alkalinization and, when excreted, urine alkalinization as well. 
Oral antacid action: Taken orally, sodium bicarbonate neutralizes stomach acid.
-Sodium carbonate is used in the manufacture of detergents, soaps, paper.
-Also used in the manufacture of water glass (sodium silicate), borax, sodium phosphate, and many other sodium compounds.

-Sodium carbonate is used in as a wetting agent in brick industry
-Sodium carbonate is used as an abrasive and foaming agent in toothpaste
-Sodium carbonate is used as a pH modifier
-Sodium carbonate is used as water softener
-Hard water which consists of magnesium and calcium ions are precipitated by carbonate.

-As a laboratory reagent to standardize acids and as an analytical reagent.
-Sodium carbonate's largest applications are in the manufacture of glass, paper, rayon, soaps and detergents. 
-As a food additive, Sodium carbonate is used as an acidity regulator, anti-caking agent, raising agent and stabiliser. 
-As a medicine, because Sodium carbonate neutralises gastric acid, Sodium carbonate acts an antacid.
-Pharma-Lubricants
-Water Treatment

-Oil & Gas
-Cleaning
-Animal Nutrition
-Coatings & Construction
-Food and Nutrition
-Agriculture
-Cosmetics
-Solvents
-Polymers
-Rubber

-Soda ash, which reduces the boiling point of silica, is a major component in glass manufacturing and has extensive application across a wide range of industries including detergents, paper, chemical and metal beneficiation (particularly chrome and vanadium).
-GLASS: Dense soda ash plays a critical role in glass production and is used as a fluxing agent, lowering the melting point of pure silica.
-CHEMICAL INDUSTRY: Dense and light soda ash are present in a large number of chemical reactions which produce the organic or inorganic compounds that are, in turn, used in a range of applications. 
For example, soda ash is used to produce sodium silicates, which are used to produce chemicals such as silica.

-DETERGENT INDUSTRY: Light soda ash is used as a binder in powdered, paste and soap detergents. 
Soda acts as a water softener and cleaning agent.
-MINING SECTOR: Soda ash is used in the beneficiation and processing of mineral ores and metals, and in the production of cobalt and steel.
-WATER TREATMENT: A source of sodium, soda ash is also used to adjust pH levels.
-NON-FERROUS METALLURGY: Soda ash is used in the recycling of zinc, aluminium and lead from spent batteries.
-FOOD INDUSTRY: As a food additive, soda ash is used to produce dyes and corn syrups, and in the manufacture of ethanol.

-TEXTILE INDUSTRY: Soda ash acts as a cleaning agent, in refining and bleaching, and to adjust the pH level during the drying process.
-Washing soda is a good all-purpose cleaner. 
Sodium carbonate's high alkalinity helps Sodium carbonate cut grease, soften water, and disinfect surfaces. 
Keep in mind that sodium carbonate solution irritates the skin and can produce chemical burns in pure form. 
-Sodium carbonate is used to adjust swimming pool pH, prevent caking in foods, and treat ringworm and eczema. 
Sodium carbonate's also used on a commercial scale for making glass and paper products.
-Heating baking soda makes Sodium carbonate transform from sodium bicarbonate into sodium carbonate, which is a stronger alkaline salt. 
Baked baking soda is useful for applications in which a strong alkaline salt is required, such as in making ramen (noodles).

-The manufacture of glass is one of the most important uses of sodium carbonate. 
Sodium carbonate acts as a flux for silica, lowering the melting point of the mixture to something achievable without special materials. 
This "soda glass" is mildly water-soluble, so some calcium carbonate is added to the melt mixture to make the glass produced insoluble. 
This type of glass is known as soda lime glass: "soda" for the sodium carbonate and "lime" for the calcium carbonate. 
Soda lime glass has been the most common form of glass for centuries.

-Sodium carbonate is also used as a relatively strong base in various fields. 
For example, Sodium carbonate is used as a pH regulator to maintain stable alkaline conditions necessary for the action of the majority of photographic film developing agents. 
Sodium carbonate acts as an alkali because when dissolved in water, Sodium carbonate dissociates into the weak acid carbonic acid and the strong alkali sodium hydroxide. 
This gives sodium carbonate in solution the ability to attack metals such as aluminium with the release of hydrogen gas.
-Sodium carbonate is a common additive in swimming pools used to raise the pH which can be lowered by chlorine tablets and other additives which contain acids.

-In cooking, Sodium carbonate is sometimes used in place of sodium hydroxide for lyeing, especially with German pretzels and lye rolls. 
These dishes are treated with a solution of an alkaline substance to change the pH of the surface of the food and improve browning.
-In taxidermy, sodium carbonate added to boiling water will remove flesh from the bones of animal carcasses for trophy mounting or educational display.
-In chemistry, Sodium carbonate is often used as an electrolyte. 
Electrolytes are usually salt-based, and sodium carbonate acts as a very good conductor in the process of electrolysis. 
In addition, unlike chloride ions, which form chlorine gas, carbonate ions are not corrosive to the anodes. 
Sodium carbonate is also used as a primary standard for acid-base titrations because Sodium carbonate is solid and air-stable, making it easy to weigh accurately.

-Domestic use:
Soda ash is used as a water softener in laundering: Soda ash competes with the magnesium and calcium ions in hard water and prevents them from bonding with the detergent being used, but does not prevent scaling. 
Sodium carbonate can be used to remove grease, oil, and wine stains.
-In dyeing with fiber-reactive dyes, sodium carbonate (often under a name such as soda ash fixative or soda ash activator) is used to ensure proper chemical bonding of the dye with cellulose (plant) fibers, typically before dyeing (for tie dyes), mixed with the dye (for dye painting), or after dyeing (for immersion dyeing).
-By far the largest consumption of sodium carbonate is in the manufacture of glass, paper, rayon, soaps, and detergents. 
Sodium carbonate is also used as a water softener, since carbonate can precipitate the calcium and magnesium ions present in "hard" water.

-Sodium carbonate is a food additive used as an acidity regulator, anticaking agent, raising agent, and stabilizer. 
Sodium carbonate is one of the components of kansui, a solution of alkaline salts used to give ramen noodles their characteristic flavor and texture. 
Sodium carbonate is also used in the production of snus (Swedish-style snuff) to stabilize the pH of the final product.
-Sodium carbonate is also used in the production of sherbet powder. 
The cooling and fizzing sensation results from the endothermic reaction between sodium carbonate and a weak acid, commonly citric acid, releasing carbon dioxide gas, which occurs when the sherbet is moistened by saliva.
-In China, Sodium carbonate is used to replace lye-water in the crust of traditional Cantonese moon cakes, and in many other Chinese steamed buns and noodles.

-Sodium carbonate is used by the brick industry as a wetting agent to reduce the amount of water needed to extrude the clay.
-In casting, Sodium carbonate is referred to as "bonding agent" and is used to allow wet alginate to adhere to gelled alginate.
-Sodium carbonate is used in toothpastes, where Sodium carbonate acts as a foaming agent and an abrasive, and to temporarily increase mouth pH.
-Sodium carbonate is used by the cotton industry to neutralize the sulfuric acid needed for acid delinting of fuzzy cottonseed.

-Sodium carbonate, in a solution with common salt, may be used for cleaning silver. 
In a nonreactive container (glass, plastic, or ceramic), aluminium foil and the silver object are immersed in the hot salt solution. 
The elevated pH dissolves the aluminium oxide layer on the foil and enables an electrolytic cell to be established. 
Hydrogen ions produced by this reaction reduce the sulfide ions on the silver restoring silver metal. 
The sulfide can be released as small amounts of hydrogen sulfide. Rinsing and gently polishing the silver restores a highly polished condition.

-Sodium carbonate is used in some aquarium water pH buffers to maintain a desired pH and carbonate hardness (KH).
-Industrial production of selenium usually involves the extraction of selenium dioxide from residues obtained during the purification of copper. 
Common production from the residue then begins by oxidation with sodium carbonate to produce selenium dioxide, which is mixed with water and acidified to form selenous acid (oxidation step).
-Sodium carbonate is commonly used in chemical reactions in the pharmaceutical industry as part of acid-base reactions. -Sodium carbonate may also be found in toothpastes as an abrasive, in water softeners used for laundry, in automatic dishwasher soaps, and some bubble bath solutions.

-Sodium carbonate is a precipitating builder, which means Sodium carbonate forms an insoluble substance that enhances or maintains the efficiency of cleansers.
-Sodium carbonate also helps control the acid-base balance of cosmetic products.
-Sodium carbonate is often used in exfoliants, toothpaste, bath oils and salts, bubble bath, moisturizers, and other products.
-When dissolved in water, sodium carbonate forms carbonic acid and sodium hydroxide — an antacid that neutralizes gastric acid.
-Sodium carbonate is also used to produce aluminum, textiles, soap, glass, and paper.

-Soda ash at the drilling rig and is used to treat most types of calcium ion contamination in freshwater and seawater muds. For cement contamination, sodium bicarbonate is used. 
-Calcium ions from drilling gypsum or anhydrite, CaSO4, cause clay flocculation and polymer precipitation and lower pH. 
-A soda-ash treatment is appropriate for gypsum contamination because caustic soda, NaOH, is not needed to raise pH. 
This is also generally the case with hard water influxes into water muds.
-Soda ash is also known as sodium carbonate, washing soda, or soda crystals. 
-Soda ash is well known for its use as a water softener in laundry, and is synthetically produced from table salt via the Solvay process.

-The Solvay process is essentially a method to create sodium carbonate from sodium chloride using recycled ammonia.
-Soda ash is a fairly strong base that can be used to maintain alkaline conditions.
-Soda ash is also used in glass manufacturing, lying (the baking of lye rolls), and taxidermy to remove flesh from bones. 
-Soda ash can also be used as an electrolyte in chemistry – Soda ash is particularly desirable because Soda ash isn’t corrosive to anodes. 
-Soda ash can be used as a standard for acid-base titrations, a descaling agent in boilers, an agent to ensure proper binding in clothing dyeing between the fiber-reactive dye and the cellulose fiber, and as a food additive (as an acidity regulator, anti-caking agent, raising agent, or stabilizer).

-Sodium carbonate can be found in powder included with ramen noodles, as well as the production of sherbet powder. 
When used as a food additive, soda ash is commonly referred to as E500 – this additive is also used in the production of Swedish snuff (known as snus) as a pH stabilizer.
-Soda ash is also used in toothpastes as a foaming agent and to raise mouth pH temporarily. 
As well as being used to clean teeth and clothing, sodium carbonate can also be found in silver cleaners.
-Soda ash can be purchased at the grocery store, as well as at swimming pool supply store or a hardware store.
-In chemistry, sodium carbonate can be used to produce sodium phosphates, sodium silicates, chrome chemicals and photographic chemicals. 
Sodium carbonate is also used in baking soda production (an ingredient in the beverage industry).

-Soda ash can also be used in lieu of caustic soda as a less expensive alternative for pH adjustment/acid neutralization, sodium chemical manufacturing, kraft pulping, and flue gas desulferization.
-Although sodium carbonate has multiple uses, in wine microbiology Sodium carbonate is mostly used as a detergent.
-Sodium carbonate is primarily used as a cleaning agent. 
Sodium carbonate's other uses are in the glass and brick industries as well as being a common additive, bonding agent and electrolyte.
-Sodium carbonate is corrosive to plastics and some metals like aluminum, lead, zinc and zinc brasses.
-Sodium carbonate is also known as washing soda and soda ash.

-Glass manufacturing
-Water softening
-pH regulation for film developing agents
-Lyeing
-Cleaning and descaling agent
-Food additive (anti-caking, acidity regulator, and stabilizer)
-Buffer substance
-PH regulator
-Filler
-Foaming agent
-Softens water
-Cleaning agent.

-Glass manufacturing is the largest application for soda ash whether Sodium carbonate is in the production of containers, fiberglass insulation, or flat glass for the housing, commercial building, and automotive industries.
-Soda ash also is used to clean the air and soften water. 
-As environmental concerns grow, demand increases for soda ash used in the removal of sulfur dioxide and hydrochloric acid from stack gases. 
-Chemical producers use soda ash as an intermediate to manufacture products that sweeten soft drinks (corn sweeteners), relieve physical discomfort (sodium bicarbonate) and improve foods and toiletries (phosphates). 

-Household detergents and paper products are a few other common examples of readily identifiable products using soda ash.
-Sodium Carbonate is used as a basimetric standard but Sodium Carbonate is not a very good primary standard since Sodium Carbonate is difficult to dry, is hygroscopic, and has a relatively low equivalent weight. 
For these reasons, Tris(hydroxymethyl)aminomethane has largely replaced Sodium Carbonate as a basimetric standard. 
Sodium Carbonate is a diequivalent base and Sodium Carbonate can be assayed by titration with a standard strong acid to the first equivalence point (pH ~ 8.3) using Phenolphthalein Indicator, or to the second equivalence point (pH ~ 3.7) using Methyl Orange Indicator. 

-The principal uses of sodium carbonate are in the manufacture of glass and the production of chemicals. 
Sodium Carbonate is also used in processing wood pulp to make paper, in making soaps and detergents, in refining aluminum, in water softening, and in many other applications. 
-Washing soda is a chemical compound that can be used to remove stubborn stains from laundry and is an essential component in most homemade laundry detergent for powder, liquid, or single pod formulas. 
Sodium Carbonate is often used in commercial detergent mixtures as well to treat hard water.

-The sodium carbonate in washing soda "softens" water helping other cleaning ingredients lift soil from the fabrics and suspend the soil in the wash water. 
The washing soda binds to the minerals which make water hard, and allows the detergent to be absorbed into fibers properly to clean clothes.
-Mainly Sodium Carbonate is used in the manufacturing of glass, paper, Rayon, Soaps, and detergents. 
-Also, Sodium Carbonate is used in the development of color on cotton and silk fabrics.

-It functions as a flux for Silica, to lower the melting point of the mixture to something achievable without special materials. 
This “soda glass” is somewhat water-soluble, so calcium carbonate is added in the melt mixture to make glass insoluble. 
Window glass (Soda-lime glass) and bottle are made by melting mixtures of sodium carbonate, silica sand, and calcium carbonate. 
When we heat these materials the carbonates release carbon dioxide. 

-Sodium Carbonate is used to soften water by removing Mg2+ and Ca2+. 
In addition, these ions form insoluble solid precipitates upon treatment with carbonate ions.
Inorganic coagulants were used to minimize carryover in cold process softening. 
In addition, effluent hardness from a cold process softener ranges 35 to 80 mg/l and for hot process softener is 10 to 40 mg/l. 
In addition, heating aids in the completion of the softening reaction, which increases the efficiency of silica removal by providing more solids to absorb silica.

-Emission of particulates from calciners and dryers are controlled with venturi scrubbers or cyclones. 
The exiting gases makes Sodium Carbonate difficult to use baghouse-type filters.
Besides, for century’s soda-lime glass was the most common form of glass in use.
-Sodium carbonate’s most important use is in the chemical make-up of glass. 
When heated at very high temperatures, combined with sand (SiO2) and calcium carbonate (CaCO3), and cooled very rapidly, sodium carbonate can be used to form a transparent non-crystalline material, commonly known as glass.
-In chemistry, sodium carbonate is often used as an electrolyte. 
This is because electrolytes are usually salt based, and sodium carbonate acts as a very good conductor in the process of electrolysis.

-Domestically Sodium Carbonate is used as a water softener during laundry. 
Sodium Carbonate competes with the ions magnesium and calcium in hard water and prevents them from bonding with the detergent being used. 
Without using washing soda, additional detergent is needed to soak up the magnesium and calcium ions. 
Called Washing Soda or Sal Soda in the detergent section of stores, Sodium Carbonate effectively removes oil, grease, and alcohol stains. 
Sodium Carbonate is also used as a descaling agent in boilers such as found in coffee pots, espresso machines, etc.

-Sodium carbonate is widely used in photographic processes as a pH regulator to maintain stable alkaline conditions necessary for the action of the majority of developing agents.
-Sodium carbonate is also used by the brick industry as a wetting agent to reduce the amount of water needed to extrude the clay.
-Soda Ash is also a common additive in municipal pools used to neutralize the acidic effects of chlorine and raise pH.
-In casting, sodium carbonate monohydrate is referred to as “bonding agent” and is used to allow wet alginate to adhere to gelled alginate.
-Sodium carbonate is often used as a primary standard for acid-base titrations because Sodium carbonate is solid and air-stable, making Sodium carbonate easy to weigh accurately.

-Sodium carbonate or also known under name of soda ash is one of the consequential raw materials in glass and detergent industries. Sodium carbonate  has a number of diversified uses that touch our lives every day. 
Glass manufacturing is the largest application for sodium carbontate whether Soda ash light is highly soluble, and therefore very useful in various manufacturing reaction processes.
-Sodium carbonate is used in the production of containers, fiberglass insulation, or flat glass for the housing, commercial building, and automotive industries.
-Soda ash light is highly soluble, and therefore very useful in various manufacturing reaction processes.

-Sodium carbonate is used in household detergents and cleaning agents such as dishwashing soaps.
-Sodium carbonate is a good option to kill fungi and other microbes. 
-In toothpaste making, manufacturers use Sodium carbonate as a foaming agent.
-Sodium carbonate is a very good fabric washer and is necessary to clean stains.
-Sodium carbonate is very important in making water glass or sodium silicate, sodium phosphate, borax, and many other compounds that contain sodium.

FOOD ADDITIVE AND COOKING of SODIUM CARBONATE:
Sodium carbonate has several uses in cuisine, largely because Sodium carbonate is a stronger base than baking soda (sodium bicarbonate) but weaker than lye (which may refer to sodium hydroxide or, less commonly, potassium hydroxide). 
Alkalinity affects gluten production in kneaded doughs and also improves browning by reducing the temperature at which the Maillard reaction occurs. 
To take advantage of the former effect, sodium carbonate is therefore one of the components of kansui, a solution of alkaline salts used to give Japanese ramen noodles their characteristic flavor and chewy texture; a similar solution is used in Chinese cuisine to make lamian, for similar reasons. 
Cantonese bakers similarly use sodium carbonate as a substitute for lye-water to give moon cakes their characteristic texture and improve browning. 
In German cuisine (and Central European cuisine more broadly), bread such as pretzels and lye rolls traditionally treated with lye to improve browning can be treated instead with sodium carbonate; sodium carbonate does not produce quite as strong a browning as lye but is much safer and easier to work with.

GLASS MANUFACTURE of SODIUM CARBONATE:
Sodium carbonate serves as a flux for silica, lowering the melting point of the mixture to something achievable without special materials. 
This "soda glass" is mildly water-soluble, so some calcium carbonate is added to the melt mixture to make the glass insoluble. 
Bottle and window glass (soda-lime glass) is made by melting such mixtures of sodium carbonate, calcium carbonate, and silica sand (silicon dioxide (SiO2)). 
When these materials are heated, the carbonates release carbon dioxide. 
In this way, sodium carbonate is a source of sodium oxide. 
Soda-lime glass has been the most common form of glass for centuries.

HYDRATES of SODIUM CARBONATE:
Sodium carbonate is obtained as three hydrates and as the anhydrous salt:
Sodium carbonate decahydrate (natron), Na2CO3·10H2O, which readily effloresces to form the monohydrate.
Sodium carbonate heptahydrate (not known in mineral form), Na2CO3·7H2O.
Sodium carbonate monohydrate (thermonatrite), Na2CO3·H2O. 
Also known as crystal carbonate.
Anhydrous sodium carbonate, also known as calcined soda, is formed by heating the hydrates. 
It is also formed when sodium hydrogencarbonate is heated (calcined) e.g. in the final step of the Solvay process.
The decahydrate is formed from water solutions crystallizing in the temperature range −2.1 to +32.0 °C, the heptahydrate in the narrow range 32.0 to 35.4 °C and above this temperature the monohydrate forms. 
In dry air the decahydrate and heptahydrate lose water to give the monohydrate. 
Other hydrates have been reported, e.g. with 2.5 units of water per sodium carbonate unit ("pentahemihydrate").

WASHING SODA:
Sodium carbonate decahydrate (Na2CO3·10H2O), also known as washing soda, is the most common hydrate of sodium carbonate containing 10 molecules of water of crystallization. 
Soda ash is dissolved in water and crystallized to get washing soda.
It is white crystalline solid;
It is one of the few metal carbonates which are soluble in water;
It is alkaline; it turns red litmus to blue;
It has detergent properties through the process of saponification which makes fats and grease water-miscible.

SYNTHESIS of SODIUM CARBONATE – Na2CO3:
Sodium carbonate is now exclusively manufactured by the Solvey process. 
In this process carbon dioxide and ammonia are passed into a cold saturated solution of sodium chloride. 
In the reactions which occur sodium hydrogen carbonate is formed which is only very slightly soluble in the presence of sodium ions, is almost completely precipitated. 
It is removed by filtration and ignited to produce sodium carbonate.
The ingredients of this process are readily available and inexpensive. 
These are salt brine (NaCl), ammonia (NH3) and limestone (CaCO3). 
In this process, CaCl2 is an important by-product obtained.
Addition of common salt to the solution containing NH4+ and HCO3– results in the precipitation of NaHCO3 which is least soluble. 
It is then filtered off.
Sodium bicarbonate is then heated to give Na2CO3.
Anhydrous sodium carbonate is dissolved in water and recrystallizes to get washing soda crystals containing 10 molecules of water of crystallization.

MAKING SODIUM CARBONATE: 
Sodium bicarbonate is CHNaO3, while sodium carbonate is Na2CO3. 
Simply heat baking soda or sodium bicarbonate in a 200 F oven for about an hour. 
Carbon dioxide and water will be given off, leaving dry sodium carbonate. 
This is the soda ash.
The compound will readily absorb water, forming the hydrate (returning to baking soda). 
Store the dry sodium carbonate in a sealed container or with a desiccant to keep Sodium Carbonate dry, or allow Sodium Carbonate to form the hydrate, as desired.
While sodium carbonate is fairly stable, Sodium Carbonate slowly decomposes in dry air to form sodium oxide and carbon dioxide. 
The decomposition reaction can be accelerated by heating the washing soda to 851 C (1124 K).

MANUFACTURE of SODIUM CARBONATE:
There are two main sources of sodium carbonate:
a)from salt and calcium carbonate (via the ammonia soda (Solvay) process)
b)from sodium carbonate and hydrogencarbonate ores (trona and nahcolite)

(a) From sodium chloride and calcium carbonate:
The overall reaction can be regarded as between calcium carbonate and sodium chloride.
However, calcium carbonate is too insoluble to react with a solution of salt.  
Instead Sodium carbonate is obtained by a series of seven stages.
The process is known as the ammonia-soda process or the Solvay process, named after the Belgian industrial chemist who patented it in 186I.
The various stages of the Solvay process are interlinked as can be seen from the diagram and description below.
(1) Ammoniation of brine:
Ammonia gas is absorbed in concentrated brine to give a solution containing both sodium chloride and ammonia. 
Na+(aq), Cl-(aq), NH4+(aq), OH-(aq) ions and NH3(aq) are present.

(2) Formation of calcium oxide and carbon dioxide:
Kilns are fed with a limestone/coke mixture (13:1 by mass).  
The coke burns in a counter-current of pre-heated air.
The heat of combustion raises the temperature of the kiln and the limestone decomposes.
The gas, containing approximately 40% carbon dioxide, is freed of lime dust and sent to the carbonating (Solvay) towers.  
The residue, calcium oxide, is used in ammonia recovery.

(3) The Solvay Tower:
This is the key stage in the process. 
The ammoniated brine from step (1) is passed down through the Solvay Tower while carbon dioxide from steps (2) and (5) is passed up it.  
The Solvay Tower is tall and contains a set of mushroom-shaped baffles to slow down and break up the liquid flow so that the carbon dioxide can be efficiently absorbed by the solution.  
Carbon dioxide, on dissolving, reacts with the dissolved ammonia to form ammonium hydrogencarbonate.
The solution now contains ions Na+(aq), Cl-(aq), NH4+(aq) and HCO3-(aq).  
Of the four substances which could be formed by different combinations of these ions, sodium hydrogencarbonate (NaHCO3) is the least soluble. 
It precipitates as a solid in the lower part of the tower, which is cooled.
A suspension of solid sodium hydrogencarbonate in a solution of ammonium chloride is run out of the base of the tower.

(4) Separation of solid sodium hydrocarbonate:
The suspension is filtered to separate the solid sodium hydrogencarbonate from the ammonium chloride solution, which is then used in stage (7).
(5) Formation of sodium carbonate:
The sodium hydrogencarbonate is heated in rotating ovens at 450 K so that it decomposes to sodium carbonate, water and carbon dioxide.
The carbon dioxide is sent back to the Solvay Tower for use in step (3).  
The product of the process, anhydrous sodium carbonate, is obtained as a fine white powder known as light sodium carbonate.

(6) Formation of calcium hydroxide:
The last two stages, (6) and (7), are concerned with the regeneration of ammonia from ammonium chloride (made in step 3).  The quicklime from step (2) is slaked with excess water giving milk of lime.
(7) Regeneration of ammonia:
This calcium hydroxide suspension is mixed with the ammonium chloride solution left from step (4) and heated.
The ammonia is thus recovered, and sent back to step (1).  
Calcium chloride is the only by-product of the whole process.
The overall process is an elegant one. 
In theory, the only raw materials are limestone and brine.  
Inevitably, there are losses of ammonia, and these are made up for by addition of extra supplies, as required in step (1).

(b) From trona and nahcolite ores:
The Solvay process is not used in the US.  
Instead, the industry uses two ores and this accounts for about 30% of the world's production.  
One is trona, found in vast amounts in Wyoming.  
The ore is mined as a solid and heated to drive off carbon dioxide, to yield sodium carbonate.
The other ore is nahcolite which is sodium hydrogencarbonate.  
On heating it forms sodium carbonate.

CHEMICAL PROPERTIES of SODIUM CARBONATE – Na2CO3
-Anhydrous sodium carbonate is stable towards heat. 
It melts without decomposition at 852oC.
-Aqueous solutions of sodium carbonate are mildly alkaline due to hydrolysis which releases OH–(aq) ions.
-Aqueous solutions of sodium carbonate absorb carbon dioxide from the air forming sodium hydrogen carbonate.
-Sodium carbonate reacts with acids like weak vegetable acids, such as lime juice liberating carbon dioxide.

SODIUM CARBONATE TEST:
The sodium carbonate test is used to distinguish between some common metal ions, which are precipitated as their respective carbonates. 
The test can distinguish between copper (Cu), iron (Fe), and calcium (Ca), zinc (Zn) or lead (Pb). 
Sodium carbonate solution is added to the salt of the metal. 
A blue precipitate indicates Cu2+ ion. 
A dirty green precipitate indicates Fe2+ ion. 
A yellow-brown precipitate indicates Fe3+ ion. 
A white precipitate indicates Ca2+, Zn2+, or Pb2+ ion. 
The compounds formed are, respectively, copper(II) carbonate, iron(II) carbonate, iron(III) oxide, calcium carbonate, zinc carbonate, and lead(II) carbonate. 
This test is used to precipitate the ion present as almost all carbonates are insoluble. 
While this test is useful for telling these cations apart, it fails if other ions are present, because most metal carbonates are insoluble and will precipitate. 
In addition, calcium, zinc, and lead ions all produce white precipitates with carbonate, making it difficult to distinguish between them. 
Instead of sodium carbonate, sodium hydroxide may be added, this gives nearly the same colours, except that lead and zinc hydroxides are soluble in excess alkali, and can hence be distinguished from calcium. 
For the complete sequence of tests used for qualitative cation analysis.

HYDRATES OF SODIUM CARBONATE:
Sodium carbonate crystallizes from water to form three different hydrates:
-sodium carbonate decahydrate (natron), Na2CO3·10H2O.
-sodium carbonate heptahydrate (not known in mineral form), Na2CO3·7H2O.
-sodium carbonate monohydrate (thermonatrite), Na2CO3·H2O.
Anhydrous sodium carbonate also known as calcined soda is formed by heating the hydrates. 
Sodium carbonate is also formed when sodium hydrogen carbonate is heated (calcined) e.g. in the final step of the Solvay process. 
The decahydrate is formed from water solutions crystallizing in the temperature range -2.1 to +32.0 C, the heptahydrate in the narrow range 32.0 to 35.4 C and above this temperature the monohydrate forms. 
In dry air the decahydrate and heptahydrate will lose water forming causing the crystals to fall apart into a white monohydrate powder. 

PHYSICAL and CHEMICAL PROPERTIES of SODIUM CARBONATE:
Molecular Weight: 105.99
Appearance Form: powder
Color: white
Color/Form: Grayish-white powder or lumps containing up to 99% sodium carbonate
Odor: odorless
Odor Threshold: Not applicable
pH: 12 at 106 g/l at 25 °C
Melting point/freezing point:
Melting point/range: 851 °C - lit.
Initial boiling point and boiling range: 1.600 °C - (decomposition)
Flash point: Not applicable
Evaporation rate: No data available
Flammability (solid, gas): 
The product is not flammable. -Flammability (solids)
Upper/lower flammability or explosive limits: No data available
Vapor pressure: No data available
Vapor density: No data available
Relative density: No data available
Water solubility: ca.212,5 g/l at 20 °C - OECD Test Guideline 105- completely soluble
Partition coefficient: n-octanol/water: Not applicable for inorganic substances
Autoignition temperature: No data available
Decomposition temperature: 400 °C -
Viscosity 
Viscosity, kinematic: No data available
Viscosity, dynamic: No data available
Explosive properties: No data available
Oxidizing properties: No data available
Boiling point: 1600 °C (decomposition)
Density: 2.52 - 2.53 g/cm3 (20 °C)
Melting Point: 851 °C
pH value: 11.16 (4 g/l, H₂O, 25 °C)
Bulk density: 1100 kg/m3
Solubility: 212.5 g/l

FIRST AID MEASURES of SODIUM CARBONATE:
-Description of first-aid measures:
General advice:
Show this material safety data sheet to the doctor in attendance.
If inhaled:
After inhalation: 
Fresh air.
In case of skin contact: 
Take off immediately all contaminated clothing. 
Rinse skin with water/ shower.
In case of eye contact:
After eye contact:
Rinse out with plenty of water. 
Call in ophthalmologist. 
Remove contact lenses.
If swallowed:
After swallowing: 
Immediately make victim drink water (two glasses at most). 
Consult a physician.

ACCIDENTAL RELEASE MEASURES of SODIUM CARBONATE:
-Personal precautions, protective equipment and emergency procedures:
Advice for non-emergency personnel: 
Avoid substance contact.
Ensure adequate ventilation. 
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Cover drains. 
Collect, bind, and pump off spills. 
Observe possible material restrictions. 
Take up dry. 
Dispose of properly. 

FIREFIGHTING MEASURES of SODIUM CARBONATE:
-Extinguishing media:
Suitable extinguishing media:
Water Foam Carbon dioxide (CO2) Dry powder
-Advice for firefighters:
In the event of fire, wear self-contained breathing apparatus.
-Further information:
Suppress (knock down) gases/vapors/mists with a water spray jet. 
Prevent fire extinguishing water from contaminating surface water or the ground water system.

EXPOSURE CONTROLS/PERSONAL PROTECTION of SODIUM CARBONATE:
-Control parameters:
Ingredients with workplace control parameters:
-Exposure controls:
Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection tested and approved under appropriate government standards such as NIOSH (US) or EN 166(EU). Safety glasses.

*Skin protection:
This recommendation applies only to the product stated in the safety data sheet, supplied by us and for the designated use. When dissolving in or mixing with other substances and under conditions deviating from those stated in EN374 please
contact the supplier of CE-approved gloves.
Full contact
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min
Splash contact
Material: Nitrile rubber
Minimum layer thickness: 0,11 mm
Break through time: 480 min

*Body Protection
protective clothing
*Respiratory protection:
Required when dusts are generated.
The entrepeneur has to ensure that maintenance, cleaning and testing of respiratory protective devices are carried out according to the instructions of the producer.
These measures have to be properly documented.
Control of environmental exposure
Do not let product enter drains.

HANDLING and STORAGE of SODIUM CARBONATE:
-Precautions for safe handling:
-Conditions for safe storage, including any incompatibilities:
Storage conditions
Tightly closed. 
Dry.
Hygroscopic

SYNONYMS:
Calcined soda
Carbonic acid disodium salt
Disodium carbonate
Carbonic acid, disodium salt
Carbonic acid sodium salt
Sodium carbonate anhydrous
Carbonic acid sodium salt (1:2)
Crystol carbonate
Natriumkarbonat
Bisodium carbonate
Soda
Natriumkarbonat
Natrum carbonicum
Sodium salt of carbonic acid
Washing soda