Sodium Chloride

F2 +2NaCl===2NaF+Cl2

Cl2 +2Na===2NaCl

2Cl2+2NaBr===2NaCl+Br2

Cl2 +2NaI ===2NaCl+I2

Cl2 +Na2S== == 2NaCl + S

Cl2 + 2NaOH == NaCl + NaClO + H2O

4Na + TiCl4 (molten) == 4NaCl + Ti

4NaH + TiCl4 == Ti + 4NaCl + 2H2

4NaH + TiCl4 == Ti + 4NaCl+2H2

NH3+NaCl+H2O+CO2==NaHCO3+NH4Cl

CO2+2NaOH (in excess)===Na2CO3+H2O

CO2+2NaAlO2+3H2O===2Al(OH)3+Na2CO3

SiO2+Na2CO3===Na2SiO3+CO2

Na2O+CO2===Na2CO3

2Na2O2+2CO2===2Na2CO3+O2

Na2CO3+HCl===NaHCO3+NaCl

3Na2CO3+ 2AlCl3+3H2O===2Al(OH)3+3CO2+6NaCl

2NaHCO3===Na2CO3+H2O+CO2

Na2O+2HCl===2NaCl+H2O

H2SO4(Concentrated)+NaCl===NaHSO4+HCl

2NaOH+Cl2===NaCl+NaClO+H2O

NaOH+HCl===NaCl+H2O

3NaOH+AlCl3===Al(OH)3+3NaCl

NaOH+NH4Cl===NaCl+NH3+H2O

Na3PO4+HCl===Na2HPO4+NaCl

Na2HPO4+HCl===NaH2PO4+NaCl

NaH2PO4+HCl===H3PO4+NaCl

Na2CO3+HCl===NaHCO3+NaCl

NaHCO3+HCl===NaCl+H2O+CO2

3Na2CO3+2AlCl3+3H2O===2Al(OH)3+3CO2+6NaCl

Sodium carbonate

CO2+2NaOH (excess)===Na2CO3+H2O

CO2+2NaAlO2+3H2O===2Al(OH)3+Na2CO3

SiO2+Na2CO3===Na2SiO3+CO2

Na2O+CO2===Na2CO3

2Na2O2+ 2CO2===2Na2CO3+O2

Na2CO3+HCl===NaHCO3+NaCl

3Na2CO3+2AlCl3+3H2O===2Al(OH)3+3CO2+6NaCl

3Na2CO3+2FeCl3+3H2O===2Fe( OH)3+3CO2+6NaCl

2NaHCO3===Na2CO3+H2O+CO2

Sodium bicarbonate

NH3+NaCl+H2O+CO2===NaHCO3+NH4Cl

CO2 (in excess) + NaOH===NaHCO3

CO2+C6H5ONa+H2O===C6H5OH+NaHCO3

Na2CO3+HCl===NaHCO3+NaCl

NaHCO3+HCl===NaCl+H2O+CO2

3NaHCO3+AlCl3===Al(OH)3+3CO2<

3NaHCO3+FeCl3===Fe(OH)3+3CO2

2NaHCO3===Na2CO3+H2O+CO2

Calcium Carbonate

CO2+Ca(OH)2 (in excess)===CaCO3+H2O

SiO2+CaCO3=== CaSiO3+CO2

2HNO3+CaCO3===Ca(NO3)2+H2O+CO2

Ca(HCO3)2===CaCO3+H2O+CO2

CaCO3===CaO+CO2

Sodium Chloride

Chemical formula NaCl, the major constituent of table and rock salt, the main component of ionic compounds. Colorless transparent cubic crystals, melting point of 801 ℃, boiling point of 1413 ℃, relative density of 2.165. Salty, easy to deliquesce when containing impurities; soluble in water or glycerol, insoluble in ethanol, insoluble in hydrochloric acid, aqueous solution neutral. Solubility in water increases slightly with the rise of temperature. When the temperature is lower than 0.15 ℃ can be obtained when the dihydrate NaCl-2H2O. sodium chloride exists in large quantities in seawater and natural salt lakes, can be used to produce chlorine, hydrogen, hydrochloric acid, sodium hydroxide, chlorate, hypochlorite, bleaching powder and sodium metal, etc., is an important chemical raw material; can be used for food flavoring and pickled fish, meat, and vegetables, as well as for the salt analysis of soaps and tanning of leather, etc.; the highly refined sodium chloride can be used The highly refined sodium chloride can be used to make physiological saline for clinical treatment and physiological experiments, such as sodium loss, water loss, blood loss and other conditions. Sodium chloride can be produced by concentrating crystallized seawater or natural salt lake or salt well water.

Name of chemical: Sodium chloride (NaCl)

Description of chemical:

Chemical formula NaCl, formula 58.44, the main component of table salt. Commonly found in white cubic crystals or fine crystalline powder. Density 2.165 g/cm3. melting point 801℃. Boiling point 1413℃. Taste salty. Soluble in water, neutral.

Use: can be used for food flavoring and pickled fish and vegetables; manufacture of chlorine, hydrogen, hydrochloric acid, sodium hydroxide, chlorate, hypochlorite, bleach, sodium metal, as well as for salting soap and tanning leather. The highly refined NaCl can be used to manufacture saline and so on. Widely used in clinical treatment and physiological experiments, such as sodium loss, water loss, blood loss and other situations. There are salt mines in nature, and a large number of them exist in seawater and salt lakes.

Method of production: produced by crystallization of concentrated seawater, but also from natural salt lakes or salt well water.

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Sodium chloride. The main ingredient in table salt. Experiments that contain more impurities are called coarse salt. Coarse salt is deliquescent due to the presence of impurities such as CaCl2\MgCl2. Saline in medicine is 0.9% sodium chloride solution.

Sodium chloride is easily soluble in water, and the solubility by the temperature change is small. 20 degrees Celsius when the solubility of 36g, 100 degrees Celsius when the solubility of 40g.

Sodium carbonate

Chemical formula Na2CO3 , white powder. Also known as soda ash, soda. Melting point 851 ℃, density 2.532 g / cm 3, hygroscopicity is very strong, it is easy to form a hard block, in the high temperature does not decompose. There are 3 kinds of sodium carbonate containing water of crystallization: Na2CO3-H2O, Na2CO3-7H2O and Na2CO3-10H2O. Sodium carbonate is easily soluble in water and is a weak acid salt that undergoes hydrolysis when dissolved in water, making the solution alkaline. Sodium carbonate in nature (such as salt lake) is called natural alkali, in ancient times has been used as a detergent and used for printing and dyeing. 1791 began to use salt, sulfuric acid, coal, limestone as raw materials for the production of sodium carbonate, is the Lubran method, the method of raw materials are not fully utilized, poor labor conditions, product quality is not good, and gradually replaced by Solvay's method. 1859 Solvay, Belgium, with salt, ammonia, carbon dioxide as the raw material, from a solution at room temperature, the production of sodium carbonate is made. In 1859, Belgium Solvay used table salt, ammonia and carbon dioxide as raw materials, precipitated sodium bicarbonate from the solution at room temperature, and heated it to decompose it into sodium carbonate, which has been used up to now. 1943, China's Hou Debeng combined with the lack of salt in mainland China to improve the Solvay method, combining the two major industries of soda ash and ammonia synthesis, and simultaneously producing sodium carbonate and fertilizer ammonium chloride, which greatly improved the utilization rate of table salt, and it is Hou's method of alkali production. Sodium carbonate is used in soap, paper, detergent production, used as a flux in the metallurgical industry, water softener.

Sodium bicarbonate

1.Chemical name:Sodium bicarbonate

2.Chemical formula:NaHCO3

3.Relative molecular mass:84

3.Chemical properties:

(1)Reaction with acid:

NaHCO3+HCl==NaCl+H20+CO2

(2)Reaction of different amount of NaHCO3 with alkali:

NaHCO3+Ca(OH)2==CaCO3+NaOH+H20

2NaHCO3+Ca(OH)2==Na2CO3+CaCO3+2H2O

3.Thermal decomposition

2NaHCO3==2NaHCO3+H2O

Calcium carbonate

The main constituent of sky-burning minerals such as marble, limestone, and chalk is calcium carbonate.

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Chemical Product Physical Properties Dictionary (Details)

Product Name Lightweight Calcium Carbonate

Product English Name Calcium carbonate, light

Calcium carbonate, light

Calcium carbonate, light light

Alias Precipitated Calcium Carbonate; Light Calcium; Precipitated Calcium Carbonate

Molecular formula CaCO3

Product use Used as a filler, used in welding rods, organic synthesis, metallurgy, glass, asbestos, pharmaceuticals, daily-use chemicals and other sectors

CAS No. 471-34-1

Toxicity protection See heavy calcium carbonate.

Packaging, storage and transportation See Activated calcium carbonate.

Physical and Chemical Properties White powder. Tasteless and odorless. There are two forms: amorphous and crystalline. Crystalline form can be divided into rhombohedral crystal system and hexagonal crystal system, columnar or rhombic. Relative density 2.71, decomposed at 825~896.6°C. Melting point is 1289°C at 10.7MPa. Difficult to dissolve in water and alcohol. Soluble in acid, while releasing carbon dioxide, exothermic reaction. Also soluble in ammonium chloride solution. Stable in air, with slight moisture absorption.

Quality standard Chemical industry standard HG/T 2226-91; National standard GB 1898-87 (food grade); Chemical industry standard HG 8257-87 (feed grade)

Molecular weight 100.09

Structural formula

Consumption quota Carbonization method

Limestone (CaCO3≥96%) 1.23

Coke (C≥80%) 0.16

Raw Coal 0.40

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Japan Carbonation method

Limestone (CaCO3) 1.20

Professional legal number

Preparation Method

Note; Reacts with acid to produce carbon dioxide, a gas that makes limewater cloudy, which is the easiest way to identify carbonate ions.

The action of insoluble calcium carbonate and water with dissolved carbon dioxide in limestone formations can be converted into calcium bicarbonate, and water with dissolved calcium bicarbonate can precipitate calcium carbonate, which is the reason for the formation of cavities.