It is the most important compound of boron. Na2B4O7 to the sodium salt of tetraboric acid.
10 It is called H2O BORAX (2). Borax can be obtained from some borates as it is found in nature as mineral Tincal (Na2B4O7 . 10 H2O), Tinkalconite (Na2B4O7 . 5 H2O) (4).
In pure form, it is in the form of colorless transparent crystals.
It loses water at 400°C. (4). R
The solution of this colorless object in water shows a mild alkaline reaction.
Therefore, borax is added to some washing powders (2).
Na+ O- O- Na+
O = B – O – B – O – B – O – B = O
Borax, sodium tetraborate
It is soluble in white water. M.N:741°C (without water)
Boric acid treated with a sodium hydroxide solution forms sodium tetraborate (Na2B4O7) solution (1).
4 H3BO3 + 2 NaOH › Na2B4O7 + 7 H2O
One of the methods used for the production of borax is based on the reaction of boric acid with Na2CO3. (So boric acid is reacted with a base.)
4 H3BO3 + Na2CO3 › Na2B4O7 + CO2 + 6 H2O
In the crystallization of borax solutions, the pentahydrate (5 H2O) is crystallized in the hot solution at temperatures above 60°C and the decahydrate (10 H2O) borax is crystallized at temperatures below.
Borax decahydrate is easily dehydrated; borax pentahydrate can be preserved better (3).
Packaging: 100 gr (0,22 lb) - 1 kg (2,20 lb) - 10 kg (22,05 lb)
Features:
Sodium borate is white and can be found in powder and crystal form.
Its density is 1.73 gr/cm3.
Sodium borate is soluble in water and glycerin. But it is insoluble in alcohol.
Borax begins to melt at 75°C.
As it melts, it loses its crystal water. It boils at 200°C.
Sodium, borate, melts in the form of a glassy mass called borax glass at red temperature.
Many metallic compounds can dissolve in the molten material, giving the borax pearl a color specific to the dissolved metallic ions.
The occurrence of colored borax pearl is used in analytical analysis to detect the presence of real metal ions such as copper, nickel, iron and chromium.
Finding:
Sodium borate is found in natural borax, which contains sodium borate along with some impurities.
Sodium borate is also obtained from many other borate minerals such as colomanite (CaB3O4(OH)3.H2O), kernite (Na2B4O7.4H2O), ulexite (Na2B4O7 Ca2B6O11.16 H2O).
Obtaining:
Sodium borate is obtained from evaporation and crystallization of salty lake waters.
Borax is obtained in the laboratory by reacting boric acid with anhydrous sodium carbonate.
Usage:
Most of the sodium borate is used in the manufacture of durable and unbreakable borosilicate glass.
Borax is also used in porcelain enamels, paints, starches and glues, and detergents.
Borax is used in bleaching laundry to remove the hardness of water, as a weld solvent and rust inhibitor.
Apart from these, borax is used in textile dyeing, printing, antifreeze to delay freezing and as a herbicide.
A small amount of boron is important for the growth of some plant types. Borax is added to the soil to eliminate infertility in the soil.
Borax can also be used as an analytical reagent in the laboratory.
Raw material information
Cas Number 1330 43 – 4
Chemical Formula Na2B4O7
Molecular Weight 201.22 GR / MOL
Trade Name BORAX ANHYDRATE
Analysis Information
Degree of Purity (%) 99
Boron Amount ( B ) ( % ) 21,25
Boiling Point ( C ) 1575
Melting Point ( C ) 741
PH Range
Density 2.360 GR / CM3
Solubility Slightly soluble in water
Physical Properties and Usage Areas
Physical appearance Crystal
Color White
Odor Odorless
Danger Causes slight irritation in contact with skin. In case of skin contact, wash with plenty of water.
Storage conditions It should be stored in a cool and moisture-free place and in closed packages.