497-19-8

Basic information

• Product Name: Sodium carbonate
• Synonyms: Bisodium carbonate;bisodiumcarbonate;Calcined;calcinedsoda;carbonatedesodium;Carbonic acid;Carbonic acid sodium salt;carbonicacid,sodiumsalt
• CAS NO: 497-19-8
• Molecular Formula: CO₃*2Na
• Molecular Weight: 105.99
• EINECS: 231-867-5
• Product Categories: Inorganics;Chromatography/CE Reagents;Eluent concentrates for ICAlphabetic;Ion Chromatography;S;SN - SZ;By Reference Material;Concentrates (e.g. FIXANAL);Reference Material Hydrochloric acidTitration;Salt Concentrates;Alphabetical Listings;Q-S;Stable Isotopes;Inorganic BasesVolumetric Solutions;Chemical Synthesis;S - ZTitration;Salt Solutions;Solution containers (VOLPAC);Synthetic Reagents;metal carbonate;Chemical Synthesis;Inorganic Bases;Materials Science;Metal and Ceramic Science;Salts;Sodium Salts;Synthetic Reagents
• Mol File: 497-19-8.mol
• Article Data: 865

Chemical Properties

• Melting Point: 851 °C(lit.)
• Boiling Point: 1600°C
• Flash Point: 169.8 °C
• Appearance: White/Solid
• Density: 2.53
• Refractive Index: 1.535
• Storage Temp.: 2-8°C
• Solubility: H2O: 1 M at 20 °C, clear, colorless
• PKA: (1) 6.37, (2) 10.25 (carbonic (at 25℃)
• Water Solubility: 22 g/100 mL (20 ºC)
• Sensitive: Hygroscopic
• Stability: Stable. Incompatible with powdered alkaline earth metals, aluminium, organic nitro compounds, fluorine, alkali metals, nonmetall
• Merck: 14,8596
• BRN: 4154566
• CAS DataBase Reference: Sodium carbonate(CAS DataBase Reference)
• NIST Chemistry Reference: Sodium carbonate(497-19-8)
• EPA Substance Registry System: Sodium carbonate(497-19-8)

Safety Data

• Hazard Codes: Xn,Xi
• Statements: 32-36-51/53-36/37/38-41-37/38
• Safety Statements: 36/37-26-22-36-39
• RIDADR: UN 3082 9/PG 3
• WGK Germany: 2
• RTECS: XN6476000
• F: 3
• TSCA: Yes
• Hazardous Substances Data: 497-19-8(Hazardous Substances Data)

Usage

Description

Sodium carbonate, Na2CO3, is a sodium salt of carbonic acid. The pure product appears as a while, odorless powder with a strong alkaline taste. It has high hygroscopicity. It can be easily dissolved in water to form an aqueous solution with moderate alkalinity. Sodium carbonate has wide applications in various kinds of fields around the world. One of most important application of sodium carbonate is for the manufacturing of glass. Based on statistics information, about half of the total production of sodium carbonate is used for the manufacturing of glass. During the production of glass, sodium carbonate acts as a flux in the melting of silica. In addition, as a strong chemical base, it is used in the manufacturing of pulp and paper, textiles, drinking water, soaps and detergents and as a drain cleaner. In addition, it can also be used for tissue digestion, dissolving amphoteric metals and compounds, food preparation as well as acting as a cleaning agent. There are generally two ways for the production of sodium carbonate. One is through the reactions between sodium chloride and calcium carbonate (via the ammonia soda (Solvay) process). The other is from sodium carbonate and hydrogencarbonate ores (trona and nahcolite).

Physical Properties

Sodium carbonate is an inorganic salt and therefore the vapour pressure can be considered negligible. It has a melting point of 851°C (CRC Handbook, 1986; The Merck Index, 1983), it decomposes when heated at > 400 °C and therefore a boiling point cannot be determined. soluble in water; insoluble in alcohol; dissolves in acids liberating CO2.The octanol water partition coefficient (log Pow) is not relevant for an inorganic substance which dissociates. The average particle size diameter (d50) of light sodium carbonate is in the range of 90 to 150 μm and of dense sodium carbonate is in the range of 250 to 500 μm. The monohydrate consists of colorless and odorless small crystals or cystalline powder; orthorhombic structure; refractive index 1.420; hardness 1.3 Mohs; density 2.25 g/cm3; loses water at 100°C becoming anhydrous; very soluble in water; insoluble in ethanol. The decahydrate consists of transparent crystals; effloresces on exposure to air; density 1.46 g/cm3; decomposes at 34°C; very soluble in water; insoluble in ethanol. An aqueous solution of sodium carbonate are strongly alkaline.

Chemical Properties

Sodium carbonate is a white, crystalline and hygroscopic powder with a purity of > 98 %. There are two forms of sodium carbonate available, light soda and dense soda. Impurities of sodium carbonate may include water (< 1.5 %), sodium chloride (< 0.5 %), sulphate (< 0.1 %), calcium (< 0.1 %), magnesium (< 0.1 %) and iron (< 0.004 %). The purity and the impurity profile depends on the composition of the raw materials, the production process and the intended use of the product. For example the purity of the pharmaceutical grade must be higher than 99.5 % in Europe. Sodium carbonate is a strong alkaline compound with a pH of 11.6 for a 0.1M aqueous solution (The Merck Index, 1983; Johnson and Swanson, 1987). The pKa of CO3 2- is 10.33, which means that at a pH of 10.33 both carbonate and bicarbonate are present in equal amounts.

Uses

Sodium carbonate is a kind of important raw material for chemical industry with wide application. It is the important raw material for making glass, soaps, detergents, textiles, leather, spices, dyes, medicines, etc. It can be used for analysis reagents and also used for the pharmaceutical industry and photoengraving. It is widely used in glass, chemicals, paper making, metallurgy, pharmaceutical, and textile as well as food industries. It is TV dedicated reagent. It can be used for the food industry as the neutralizing agent, leavening agents such as for the manufacture of amino acids, soy sauce and pasta such as bread, bread and so on. It can also be prepared to dubbed alkaline and add into pasta to increase the flexibility and ductility. As the detergent, it can be used for wool rinse. It can also be applied to bath salts and pharmaceutical use and also be used as the alkali agent of tanning. Sodium carbonate is most used in industry with a small part using by the civilian. In the soda ash of industry purpose, it is mainly applied to light industry, building materials and chemical industry, accounting for about 2/3: followed by metallurgy, textiles, petroleum, defense, and pharmaceutical. The glass industry is the largest soda consumer sector with each ton of glass consuming 0.2 ton of soda ash. In the chemical industry, it can be used for manufacturing of sodium silicate, sodium dichromate, sodium nitrate, sodium fluoride, baking soda, borax, and trisodium phosphate. In the metallurgical industry, it is mainly used for fluxing agent, mineral flotation agent, and desulfurization agent for steel and antimony. It can also be used as water softener in printing and dyeing industry. In tanning industry, it can be used for the degreasing of raw hides, neutralizing chrome tanned leather and improving the alkalinity of the chrome liquid. It is also used in the production of synthetic detergent additive sodium tripolyphosphate and other sodium salt. It can be used as a buffer, neutralizing agent and dough conditioner. It can be used in cakes and pastas. Make appropriate use it according to actual requirement of production. It is mainly applied to float glass, funnels, optical glass. It can also be used in other sectors of chemical industry and metallurgy industry. It can reduce the flying the alkali dust through application of heavy soda ash, and thus reducing the material consumption, improving the working conditions as well as improving product quality while reducing its erosion on the refractory material to extend the life of the furnace. It is a kind of basic chemical raw material which is widely used in medicine, paper making, metallurgy, glass, textiles, dyes and other industries and can be used as a leavening agent in food industry. It can be used as analytical reagents, dehydrating agent, and battery additives.

Biological Functions

Sodium carbonate is used as a buffer component in such applications as chromatography, capillary electrophoresis, and enzyme catalysis. Sodium carbonate is widely used in the isolation of cell membranes, membrane proteins, and hydrophobic proteins. A protocol for the isolation of polyamines from cell culture media has been published.

Toxicity

ADI (acceptable daily intake) make no restrictions (FAO/WHO in 1985). LD50 (median lethal dose) is about 6 g/kg (mice-oral). Soda ash dust has irritation effects on the skin, respiratory and eyes. Long-term exposure to soda solution may cause eczema and dermatitis. Its concentrated solutions can cause burns, necrosis, and even corneal opacity. The maximal allowable concentration of soda ash dust in the air is 2 mg/m3. The operators should wear overalls, door cover, gloves, boots and other protective clothing to protect the respiratory system and skin.

Production method

Sodium carbonate at present is mostly mined from its natural deposits. It also is manufactured syntheticallly by Solvay (or ammonia-soda) process. The natural production of sodium carbonate currently has supassed its synthetic production. The Solvay process involves a series of partial reactions. The first step is calcination of calcium carbonate to form lime and CO2. Lime is converted to calcium hydroxide. The most crucial step of the process involves reacting brine solution with carbon dioxide and ammonia to produce sodium bicarbonate and ammonium chloride. Sodium bicarbonate converts to sodium carbonate. The calcium hydroxide and ammonium chloride react to form calcium chloride as the by-product. The partial reactions are shown below: CaCO3 → CaO + CO2 CaO + H2O → Ca(OH)2 2NaCl + 2CO2 + 2NH3 + 2H2O → 2NaHCO3 + 2NH4Cl 2NaHCO3 → Na2CO3 + H2O + CO2 Ca(OH)2 + 2NH4Cl → CaCl2 + 2NH3 + 2H2O The overall reaction: CaCO3 + 2NaCl → Na2CO3 + CaCl2 Sodium carbonate was made historically by the Leblanc process. The first commercial production was carried out by the Leblanc process. In this process, sodium chloride was treated with sulfuric acid to produce sodium sulfate and hydrochloric acid. Heating the sodium sulfate with coal and limestone produced a “black ash” that contained sodium carbonate, calcium sulfide, unreacted coal, and calcium carbonate. Sodium carbonate was separated from the black ash by leaching with water. The overall reaction is as follows: Na2SO4 + 2C + CaCO3 → Na2CO3 + CaS + 2CO2

References

https://en.wikipedia.org/wiki/Sodium_hydroxide#Uses http://www.essentialchemicalindustry.org/chemicals/sodium-carbonate.html

Description

Sodium carbonate is known as soda ash or washing soda and is a heavily used inorganic compound. Approximately 45 million tons of soda ash are produced globally both naturally and synthetically. Soda ash is obtained naturally primarily from the mineral trona, but it can also be obtained from nahcolite (NaHCO3) and salt brine deposits. Trona is a freshwater sodium carbonate-bicarbonate evaporite, with the formula Na3CO3HCO3 .2H2O. The largest known deposit of trona is located in the Green River area of Wyoming, and other large deposits are found in Egypt’s Nile Valley and California’s Searles basin around the city of Trona. Soda ash is produced from mined trona by crushing and screening the ore and then heating it. Th is produces a soda ash mixed with impurities. Pure soda ash is obtained by dissolving the product and precipitating impurities combined with filtering processes.

Chemical Properties

Sodium carbonate, Na2C03, also known as soda or soda ash,is the most important of the industrial alkalis. It is a white or grayish-white, lumpy, water-soluble powder that loses its water of crystallization when heated. It decomposes at a temperature of about 852°C (1560°F). It exists in solution only. It is prepared by the combination of carbon dioxide and water.

Occurrence

Ash is a tree found in regions of North America

History

Sodium carbonate, Na2CO3, has been used historically for making glass, soap, and gunpowder. Along with potassium carbonate, known as potash, sodium carbonate was the basis of the alkali industry, which was one of the first major chemical industries. Throughout history, alkalis were obtained from natural sources. Soda ash was also produced by burning wood and leaching the ashes with water to obtain a solution that yielded soda ash when the water was boiled off. The name soda ash originates from the barilla plant, which was used to produce soda ash. The scientific name of this plant is Salsola soda, but it goes by the common names of sodawort or glasswort because the soda produced from it was used in making glass. Barilla is a common plant found in saline waters along the Mediterranean Sea in Spain and Italy. Barilla was dried and burned to produce soda ash. The depletion of European forests and international disputes made the availability of alkali salts increasingly uncertain during the latter part of the 18th century. LeBlanc proposed a procedure in 1783, and a plant based on LeBlanc’s method was opened in 1791. Unfortunately, LeBlanc’s association with French Royalty led to the confi scation of the plant at the time of the French Revolution. Furthermore, confl icting claims for LeBlanc’s method were made by several other chemists and he never received the reward.

Uses

Soda ash is used in glass making, in production of sodium chemicals (such as sodium chromates, phosphates, and silicates), in the wood pulp industry, in production of soaps and detergents, in oil refining, in water softening, and in refining of nonferrous metals. In its hydrous crystallized form (Na2C03.10H2O), it is known as sal soda,washing soda,or soda crystals, not to be confused with baking soda,which is sodium hydrogen carbonate or sodium bicarbonate (NaHC03). Its monohydrate form(Na2C03·H20) is the standard compound for scouring solutions. When in solution, sodium carbonate creates less alkalinity than the hydroxides. A 0.1% solution creates a pH of 11;a fully saturated solution is 35%, which has a pH of 12.5. The safety requirements for sodium carbonate, because of its lower alkalinity, can be considered less demanding than those for the related bicarbonates.

Uses

Sodium Carbonate is an alkali that exists as crystals or crystalline powder and is readily soluble in water. it has numerous functions: an antioxidant, a curing and pickling agent, a flavoring agent, a processing aid, a sequestrant, and an agent for ph control. it is used in instant soups to neutralize acidity. it is used in alginate water des- sert gels to sequester the calcium, allowing the alginate to solubilize. it is also used in puddings, sauces, and baked goods.

Uses

Sodium carbonate is also known as washing soda or carbonate of soda, sodium carbonate is a white crystal or powder made by converting salt into sodium sulfate, which was followed by roasting with limestone and coal. It is soluble in water and glycerin but not alcohol. Sodium carbonate was used as a pH modifier in toning baths and as the primary alkali in developers used for gelatin emulsions.

Definition

A dibasic acid formed in small amounts in solution when carbon dioxide dissolves in water: CO2 + H2O?H2CO2 It forms two series of salts: hydrogencarbonates (HCO3–) and carbonates (CO32-). The pure acid cannot be isolated.

Definition

sodium carbonate: Anhydrous sodium carbonate (soda ash, sal soda) is a white powder, which cakes and aggregates on exposure to air due to the formation of hydrates. The monohydrate, Na2CO3·H2O, is a white crystalline material, which is soluble in water and insoluble in alcohol; r.d. 2.532; loses water at 109°C; m.p. 851°C.The decahydrate, Na2CO3·10H2O (washing soda), is a translucent ef?orescent crystalline solid; r.d. 1.44; loses water at 32–34°C to give the monohydrate; m.p. 851°C.Sodium carbonate may be manufactured by the Solvay process or by suitable crystallization procedures from any one of a number of natural deposits, such as:trona (Na2CO3·NaHCO3·2H2O),natron (Na2CO3·10H2O),ranksite (2Na2CO3·9Na2SO4·KCl),pirsonnite (Na2CO3·CaCO3·2H2O),gaylussite (Na2CO3·CaCO3·5H2O).The method of extraction is very sensitive to the relative energy costs and transport costs in the region involved. Sodium carbonate is used in photography, in cleaning, in pH control of water, in textile treatment, glasses and glazes, and as a food additive and volumetric reagent.

Production Methods

Sodium carbonate is produced on all continents of the world from its minerals. It is present in large deposits in Africa and the United States as either carbonate or trona, a mixed ore of equal molar amounts of carbonate and bicarbonate. However, about 70% of the world production of sodium carbonate is manufactured by the Solvay (ammonia soda) process, whereby ammonia is added to a solution of sodium chloride. Carbon dioxide is then bubbled through to precipitate the bicarbonate (NaHCO3) that is decomposed by heat-producing sodium carbonate. In the United States. all production is based on the minerals that contain sodium carbonate. Different qualities of sodium carbonate are produced: technical, food, and pharmaceutical grades.

General Description

Sodium carbonate is a water soluble inorganic salt commonly used as a weak base. Its aqueous solution has the ability to uptake carbon dioxide. It can also catalyze the conversion of sewage sludge to liquid fuels.

Flammability and Explosibility

Nonflammable

Biochem/physiol Actions

Buffer component, may be used for the removal of peripheral membrane proteins.

Safety Profile

Poison by intraperitoneal route. Moderately toxic by inhalation and subcutaneous routes. Mlldly toxic by ingestion. Experimental reproductive effects. A skin and eye irritant. It migrates to food from packagmg materials. Can react violently with Al, P2O5, H2SO4, F2, Li, 2,4,6-trinitrotoluene. When heated to decomposition it emits toxic fumes of Na2O

Purification Methods

It crystallises from water as the decahydrate which is redissolved in water to give a near-saturated solution. By bubbling CO2, NaHCO3 is precipitated. It is filtered off, washed and ignited for 2hours at 280o [MacLaren & Swinehart J Am Chem Soc 73 1822 1951]. Before being used as a volumetric standard, analytical grade material should be dried by heating at 260-270o for 0.5hour and allowed to cool in a desiccator. It has a transition point at 450o, and its solubility in water is 21.58% at 20o (decahydrate in solid phase), 49.25% at 35o (heptahydrate in solid phase) and 44.88% at 75o(monohydrate in solid phase) [D.nges in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I p 987-988 1963]. After three recrystallisations, technical grade Na2CO3 had Cr, Mg, K, P, Al, W, Sc and Ti at 32, 9.4, 6.6, 3.6, 2.4, 0.6, 0.2 and 0.2 ppm respectively; another technical source had Cr, Mg, Mo, P, Si, Sn and Ti at 2.6, 0.4, 4.2, 13.4, 32, 0.6, 0.8 ppm respectively.

InChI:InChI=1/CH2O3.2Na/c2-1(3)4;;/h(H2,2,3,4);;/q;2*+1/p-2

Synthetic route

ammonium carbonate + ammonia (7664-41-7) + sodium chloride (7647-14-5) → sodium carbonate (497-19-8)

Conditions	Yield
In water NH3 passed into a soln. of (NH4)2CO3-NaCl until satn.; product free of Cl and NH3;	100%
In water NH3 passed into a soln. of (NH4)2CO3-NaCl until satn.; product free of Cl and NH3;	100%

Na2[B(CN)3] + water (7732-18-5) + potassium carbonate (584-08-7) → K[HB(CN)3] + sodium carbonate (497-19-8) + sodium hydroxide (1310-73-2)

Conditions	Yield
With tetrahydrofuran	A 100% B n/a C n/a

Glauber's salt + carbon monoxide (201230-82-2) + hydrogen (1333-74-0) → hydrogen sulfide (7783-06-4) + water (7732-18-5) + sodium carbonate (497-19-8)

Conditions	Yield
with molten Na2SO4*10H2O; heating at 927 to 983°C for 2 h; ratio of CO and H2 1:3;	A 98% B n/a C n/a

carbon monoxide (201230-82-2) + water (7732-18-5) + sodium sulfate (7757-82-6) → sodium carbonate (497-19-8)

Conditions	Yield
iron(III) oxide In neat (no solvent) passing a mixture of CO/H2O-vapor over powdered Na2SO4 at 660°C; partial pressure of H2O: 0.3 at, catalyst: Fe2O3 in form of a Fe(NO3)2-soln.;; 85-92% Na2CO3;;	97%
With catalyst: Fe2O3 and Sb2O5 or Fe2O3 and Sb2O4 or; Fe2O3 and As2O5 In neat (no solvent) passing a mixture of CO/H2O-vapor (CO from passing air through hot charcoal) over Na2SO4; partial pressure of H2O: 0.4 at, gas, containing 14.6% CO, is applied in 1.5-fold excess; catalyst: mixture of Fe2O3 and Sb2O5, Sb2O4 or As2O5;; 88.5% Na2CO3;;	93.8%
With catalyst: Fe2O3 and Sb2O5 or Fe2O3 and Sb2O4 or; Fe2O3 and As2O5 In neat (no solvent) passing a mixture of CO/H2O-vapor (CO from passing air through hot charcoal) over Na2SO4, partial pressure of H2O: 0.4 at, catalyst :mixture of Fe2O3 and Sb2O5, Sb2O4 or As2O5;; 91.3-95.6% Na2CO3;;	94-97.6

N-Cyanoguanidine (127099-85-8, 780722-26-1) + sodium hydroxide (1310-73-2) → disodium cyanamide + sodium carbonate (497-19-8)

Conditions	Yield
after V. A. Shushunov and A. M. Pavlov, Dokl. Akad. Nauk SSSR, 89, 1033(1953);	A 95% B 5%

disodium tetracarbonylferrate + carbon dioxide (124-38-9) → iron pentacarbonyl (13463-40-6) + sodium carbonate (497-19-8)

Conditions	Yield
In tetrahydrofuran reductive disproportionation, mechanism discussed;; IR; iron carbonyl not isolated;;	A 82% B 94%

sodium formate (141-53-7) → sodium oxalate (62-76-0) + sodium carbonate (497-19-8)

Conditions	Yield
sodium hydroxide In solid byproducts: H2; with NaOH (1:0.05) in N2 atmosphere, the heating rate 6 deg/min;	A 92% B n/a
In solid thermal decomposition of sodium formate in H2 atmosphere (TG at 435 :degree.C, the heating rate 6 deg/min;	A 35% B n/a
In solid thermal decomposition of sodium formate in CO atmosphere (TG at438 °C), the heating rate 6 deg/min;	A 34% B n/a

disodium tetracarbonylosmate + carbon dioxide (124-38-9) + iodine (7553-56-2) → cis-Os(CO)4(I)2 (17632-05-2) + sodium carbonate (497-19-8)

Conditions	Yield
In tetrahydrofuran addn. of CO2 to suspension of Na2(Os(CO)4) in THF, filtn. onto I2 at 4°C;; pptg. of carbonate; soln.: removal of solvent (IR), sublimation off excess I2, extn. into toluene and concg. under vacuum;;	A 61% B 92%

(R)-phenylglycine (875-74-1) + methyl chloroformate (79-22-1) → sodium carbonate (497-19-8)

Conditions	Yield
With sodium hydroxide In water at 0℃; for 1h;	91%

carbon dioxide (124-38-9) → sodium carbonate (497-19-8)

Conditions	Yield
With [(1,1,4,7,10,10-hexamethyltriethylenetetramine)(Fe(NO)2)2]; sodium In tetrahydrofuran at 20℃; under 760.051 Torr; for 72h; Glovebox; Inert atmosphere; Sealed tube;	90%
With Na-silicate In water introduction of CO2 into the aq. soln.;;
With Na-aryl sulfonate In further solvent(s) byproducts: aryl sulfonic acid ester; dissolving Na-aryl sulfonate (from aryl sulfonic acid and NaCl) in an alcohol, introduction of CO2-gas;;

sodium sulfate (7757-82-6) + barium carbonate → sodium carbonate (497-19-8)

Conditions	Yield
In water byproducts: BaSO4; wt.-ratio Na2SO4:BaCO3=5:11, 7h. at 33.+-.1°C;;	88.97%
With Ba(HCO3)2 In not given reaction of a soln. of BaCO3 with Na2SO4; complete reaction by addition of a small amount of Ba(HCO3)2;;

sodium tetrahydroborate (16940-66-2) + sodium formate (141-53-7) → sodium oxalate (62-76-0) + sodium carbonate (497-19-8)

Conditions	Yield
In solid reaction of sodium formate with NaBH4 (1:0.05) in N2 atmosphere, the heating rate 6 deg/min;	A 88% B n/a
In solid reaction of sodium formate with NaBH4 (1:1) in N2 atmosphere, the heating rate 6 deg/min;	A 0% B n/a

sodium sulfate (7757-82-6) + calcium carbonate → sodium carbonate (497-19-8)

Conditions	Yield
With pyrographite In neat (no solvent) Leblanc process: heating; Na2SO4:CaCO3:C=100:100:75;;	88%
In melt	0%
In water Electrolysis; electrolysis of Na2SO4 soln. with an inert anode covered with a layer of insoluble CaCO3; reaction of CaCO3 with formed H2SO4 forming CO2; reaction of CO2 with NaOH formed in the cathod region;;
In melt	0%
In water

2Na(1+)*W(CO)5(2-) = Na2[W(CO)5] (54099-82-0) + carbon dioxide (124-38-9) → tungsten hexacarbonyl (14040-11-0) + sodium carbonate (497-19-8)

Conditions	Yield
In tetrahydrofuran reductive disproportionation; mechanism discussed;; IR;;	A 83% B n/a
In tetrahydrofuran soln. of the W-compound was treated with gasous CO2 at -78°C, warmed to 25°C; solvent removed (vac.), extd. (diethyl ether), ether removed (vac.); IR, MAS;	A 83% B n/a

sodium tetracarbonylruthenate(II) + carbon dioxide (124-38-9) + iodine (7553-56-2) → cis-{RuI2(CO)4} (15663-30-6, 18475-75-7, 25322-72-9) + sodium carbonate (497-19-8)

Conditions	Yield
In tetrahydrofuran bubbling of excess CO2 through a suspension of Na2(Ru(CO)4) in THF (stirred 20min, 4°C), filtration of soln. onto I2 at 4°C;; pptg. of carbonate; soln.: removal of solvent (IR), sublimation off of excess iodine, extn. with THF;;	A 73% B 61%

2Na(1+)*{V(C5H5)(CO)3}(2-)*C4H8O=Na2{V(C5H5)(CO)3}*C4H8O + carbon dioxide (124-38-9) → tetracarbonyl(η(5)-cyclopentadienyl)vanadium(I) + sodium carbonate (497-19-8)

Conditions	Yield
In tetrahydrofuran bubbling of gaseous CO2 through suspension of corresponding carbonyl complex in THF for 5min at room temp.;; IR; removal of excess CO2 under vacuum, concg., extraction with pentane, concg. under reduced pressure; pentane insol. ppt.: carbonate;;	A 67% B 57%

sodium hexaflorophosphate + [Fe(η5-cyclopentadienyl)(η-benzene)] + carbon dioxide (124-38-9) + trimethylphosphane (594-09-2) → {Fe(cp)(PMe3)3}(PF6) + {Fe(cp)(PMe3)2CO}(PF6) + sodium carbonate (497-19-8)

Conditions	Yield
CO2 reacts with (Fe(cp)(C6H6)) (1 atm, 0°C) in presence of PMe3 and NaPF6 to (Fe(cp)(PMe3)3)PF6;	A 66% B 33% C n/a

selenium (7782-49-2) → sodium selenate + sodium carbonate (497-19-8) + sodium hydroxide (1310-73-2)

Conditions	Yield
With sodium peroxide In neat (no solvent) byproducts: Na2SO4; oxidation of Se on melting with Na2O2in a Ni crucible;; the formed melt contains NaOH and Na2CO3; isolation as mixture of Na2SeO4 and Na2SO4;;	A 58% B n/a C n/a
With Na2O2 In neat (no solvent) byproducts: Na2SO4; oxidation of Se on melting with Na2O2in a Ni crucible;; the formed melt contains NaOH and Na2CO3; isolation as mixture of Na2SeO4 and Na2SO4;;	A 58% B n/a C n/a

sodium acetate (127-09-3) → sodium carbonate (497-19-8) + pyrographite (7440-44-0) + acetone (67-64-1)

Conditions	Yield
In neat (no solvent) decomposition at 390°C, formation of acetone, Na2CO3 and traces of C between 410 and 450°C while distilling;;	A n/a B <1 C 53%
In neat (no solvent) decomposition at 390°C, formation of acetone, Na2CO3 and traces of C between 410 and 450°C while distilling;;	A n/a B <1 C 53%

sodium formate (141-53-7) + lithium hydroxide (1310-65-2) → sodium oxalate (62-76-0) + sodium carbonate (497-19-8)

Conditions	Yield
In solid byproducts: H2; reaction of sodium formate with LiOH (1:0.05) in N2 atmosphere, the heating rate 6 deg/min;	A 49% B n/a

dinatriumdecacarbonylwolframate → triphenylphosphine tungsten pentacarbonyl (15444-65-2) + sodium formate (141-53-7) + sodium hydrogencarbonate (144-55-8) + sodium carbonate (497-19-8)

Conditions	Yield
With carbon dioxide; triphenylphosphine In acetonitrile Irradiation (UV/VIS); (Ar or N2); UV irradn. (>420 nm) of soln. of W compd. and PPh3 with stirring at ca. 20°C for ca. 12 h under CO2 pressure, formed ppt. was sepd.; W(CO)5PPh3 was detected IR spect. in filtrate, not isolated; NaHCOO detected 1HNMR spect. in D2O soln. of ppt.; Na2CO3 and NaHCO3 detd. in aq. soln. of ppt. by titrn.;	A 70-90 B 20% C 18% D 39%

Na(1+)*H(1+)*W2(CO)10(2-)=NaHW2(CO)10 → triphenylphosphine tungsten pentacarbonyl (15444-65-2) + trans-triphenylphosphane tetracarbonyltungsten (16743-03-6, 38800-77-0, 68738-00-1) + sodium formate (141-53-7) + sodium hydrogencarbonate (144-55-8) + sodium carbonate (497-19-8)

Conditions	Yield
With carbon dioxide; triphenylphosphine In acetonitrile Irradiation (UV/VIS); (Ar or N2); UV irradn. (>420 nm) of soln. of W compd. and PPh3 with stirring at ca. 20°C for ca. 12 h under CO2 pressure, formed ppt. was sepd.; W compds. were detected IR spect. in filtrate, not isolated; NaHCOO detected 1HNMR spect. in D2O soln. of ppt.; Na2CO3 and NaHCO3 detd. in aq. soln. of ppt. by titrn.;	A n/a B n/a C 30% D 29% E 27%

ammonia (7664-41-7) + amino-guanidine; compound with copper (II)-nitrate → sodium carbonate (497-19-8)

water (7732-18-5) + copper(II) methylsalicylate dihydrate → sodium carbonate (497-19-8) + methyl salicylate (119-36-8) + copper hydroxide

Conditions	Yield
Hydrolysis;

edetate disodium (139-33-3) → carbon dioxide (124-38-9) + sodium carbonate (497-19-8) + NaNO3

Conditions	Yield
With ozone at 20℃; Mechanism; Rate constant; Thermodynamic data; variation in pH, acidity of solution, and temperature; activation energy;

alpha-D-glucopyranose (492-62-6) → ethanol (64-17-5) + sodium glycolate (25289-18-3, 105938-46-3, 2836-32-0) + sodium carbonate (497-19-8) + sodium lactate (312-85-6)

Conditions	Yield
With sodium hydroxide at 145℃; for 1h; Product distribution;

sodium L-(+)-lactate → ethanol (64-17-5) + sodium carbonate (497-19-8) + sodium lactate (312-85-6)

Conditions	Yield
With sodium hydroxide at 145℃; for 1h; Product distribution;

1-13C-sodium-L-lactate → ethanol (64-17-5) + sodium carbonate (497-19-8) + sodium lactate (312-85-6)

Conditions	Yield
With sodium hydroxide at 145℃; for 1h; Product distribution;

Upstream product

• 533-96-0 SODIUM SESQUICARBONATE DIHYDRATE 
• 10294-33-4 Boron tribromide 
• 1313-82-2 Sodium sulfide 
• 1313-84-4 SODIUM SULPHIDE HYDRATE 
• 1317-65-3 CALCIUM CARBONATE 
• 104-88-1 4-Chlorobenzaldehyde 
• 124-38-9 CARBON DIOXIDE 
• 113-24-6 Sodium pyruvate 
• 123-31-9 Hydroquinone 
• 144-55-8 Sodium bicarbonate 
• 471-34-1 Calcium carbonate 
• 5968-11-6 SODIUM CARBONATE, MONOHYDRATE 
• 7647-14-5 Sodium chloride 
• 7727-73-3 SODIUM SULFATE DECAHYDRATE 

Downstream Products

• 13036-57-2 2-Chloro-4-methylpyrimidine 
• 3068-88-0 BETA-BUTYROLACTONE 
• 479-41-4 Indirubin 
• 4191-73-5 Isopropylparaben 
• 13472-35-0 Sodium dihydrogen phosphate dihydrate 
• 1609-86-5 tert-Butylisocyanate 
• 1594-58-7 3-PYRIDYLAMIDOXIME 
• 1698-54-0 3-HYDROXY-1-PHENYL-6-PYRIDAZONE 
• 1772-01-6 N'-HYDROXYPYRIDINE-2-CARBOXIMIDAMIDE 
• 112-14-1 Acetic acid octyl ester 
• 123333-67-5 SODIUM HYPOPHOSPHITE MONOHYDRATE 
• 101-39-3 alpha-Methylcinnamaldehyde 
• 612-25-9 2-Nitrobenzyl alcohol 
• 613-92-3 BENZAMIDOXIME HYDROCHLORIDE 
• 534-16-7 Silver carbonate 
• 107-04-0 1-Bromo-2-chloroethane 
• 1594-57-6 N'-HYDROXYPYRIDINE-4-CARBOXIMIDAMIDE 
• 504-08-5 2,4-DIAMINO-1,3,5-TRIAZINE 
• 56-04-2 Methylthiouracil 
• 96-21-9 1,3-Dibromo-2-propanol 
• 109-59-1 2-ISOPROPOXYETHANOL 
• 53370-51-7 N'-HYDROXY-2-THIOPHENECARBOXIMIDAMIDE 
• 159709-60-1 N-(Ethoxycarbonyl)-4-ethoxycarbonyl-1-methylpyrazole-5-sulfonamide 
• 13767-89-0 GLAUBERITE 
• 8048-16-6 Streptodornase/streptokinase 
• 13775-52-5 Aluminate(3-),hexafluoro-, potassium (1:3), (OC-6-11)- 
• 57-68-1 Sulfamethazine 
• 868-18-8 Sodium tartrate 
• 6328-58-1 6-Methyl-2-(methylthio)pyrimidin-4-ol 
• 17095-24-8 REACTIVE BLACK 5 

Recommend Products

• 123-91-1  1,4-dioxane 
• 41441-40-1  ethyl 3-phenyl-4-nitrobutanoate 
• 191-28-6  perixanthenoxanthene 
• 110-86-1  pyridine 
• 98-95-3  nitrobenzene 
• 602-09-5  1,1'-bi-2-naphthol 
• 98-01-1  furfural 
• 98-00-0  (2-furyl)methyl alcohol 
• 91-22-5  quinoline 
• 99-65-0  meta-dinitrobenzene 
• 119-61-9  benzophenone 
• 91-01-0  1,1-Diphenylmethanol 
• 5392-40-5  (E/Z)-3,7-dimethyl-2,6-octadienal 
• 106-24-1  Geraniol