Sodium perborate tetrahydrate

Commercial preparation of sodium perborate tetrahydrate is by reaction of a sodium metaborate solution, from sodium hydroxide and borax pentahydrate, and hydrogen peroxide followed by crystallization of tetrahydrate (95). The tnhydrate and monohydrate can be formed by reversible dehydration of the tetrahydrate. 

In a 1-1. three-necked round-bottomed flask equipped with an eflicient stirrer, a reflux condenser, and a thermometer (Note 1) are placed 500 ml. of glacial acetic acid (Note 2), 29.0 g. (0.19 mole) of -aminoacetanilide (Note 3), 40 g. (0.26 mole) of sodium perborate tetrahydrate, and 10 g. (0.16 mole) of boric acid. The mixture is heated with stirring to 50-60° and held at this temperature for 6 hours. Initially the solids dissolve but, after heating for approximately 40 minutes, the product begins to separate. At the end of the reaction period, the mixture is cooled to room temperature and the yellow product is collected on a Buchner funnel. It is washed with water until the washings are neutral to pH paper (Note 4) and then dried in an oven at 110°. The yield of 4,4 -bis(acetamido)a2obenzene, m.p. 288-293° (dec.), is 16.5 g. (57.7%). It is used as such for the hydrolysis step (Note 5). 

The dominant bleaches in Europe and many other regions of the world are of the peroxide variety. The usual sources of hydrogen peroxide are inorganic peroxides and peroxohydrates. The most frequently encountered source is sodium perborate tetrahydrate. Sodium perborate monohydrate and sodium percarbonate have been increasingly used at the expense of sodium perborate tetrahydrate. 

Sodium perborate monohydrate Sodium perborate tetrahydrate Sodium percarbonate Sodium perchlorate Sodium perchlorate monohydrate Sodium permanganate Sodium peroxide Sodium persulfate Strontium chlorate Strontium perchlorate Strontium peroxide Tetranitromethane Thallium chlorate Trichloro-s-triazinetrione (trichloroisocyanuric) (acid all forms)... 

Yiiksel, G.Y., Titiz, S., and Bulutcu, A.N. Solubility of sodium perborate tetrahydrate in water and sodinm metaborate solutions, J. Chem. Eng. Data, 41(3) 586-588, 1996. 

Experimental Materials. Sodium perborate tetrahydrate (NaB02 4H20) was obtained from Alfa Products titration for available H2O2 by KMnO gave > 95% of theoretical equivalency. 

SAMP-Hydrazones derived from ketones may also be cleaved by treatment with three equivalents of sodium perborate tetrahydrate at pH 7 in water/rert-butyl alcohol at 60 °C. Hydrolysis of aliphatic derivatives is effected in 4-24 hours and reactions yielding aromatic ketones proceed within 2- 3 days. This cleavage reaction furnishes the desired ketones chemoselectively in the presence of olefinic double bonds in 85-95% yield (cyclopentanone 70% yield)30. 

Sodium Carbonate Peroxyhydrate. Sodium carbonate peroxyhydrate [15630-89-4], which contains about 14 wt % of active oxygen, has the composition 2Na C(% 3H202. A white, free-flowing solid, it generally can be used in all applications where perborate is used. Despite the fact that sodium carbonate peroxyhydrate has a greater rate of dissolution than sodium perborate tetrahydrate, the latter is usually favored for its good storage stability and better compatibility with the various materials used in formulations (79). 

Marlon ARL B.O Sodium soap powder 3.0 Sodium tripolyphosphate 30.0 Sodium disilicate 9-0 Sodium perborate tetrahydrate 20.0 Tetraacetyethylenediamine (TAED) 3.0 Carboxymethy1 cellulose 1-0 Sodium sulphate light, enzymes to 100... 

Savizky, R. M., Suzuki, N. and Bove, J. L. The use of sonochemistry in the asymmetric epoxidation of substituted chalcones with sodium perborate tetrahydrate. Tetrahedron Asymmetry, 1998, 9, 3967-3969. 

Sodium perborate tetrahydrate (770 mg, 5 mmol), was added to a stirred solution of the iodoarene (1 mmol) in a mixture of hydrochloric acid (20 ml) and either acetonitrile or carbon tetrachloride (20 ml) the latter was more effective for all three iodoanisoles. The mixture was stirred at room temperature for 2 h (with the exception of p-diiodobenzene which required 3 days) and then was diluted with water (100 ml). The resulting solid which separated was collected, washed with water and light petroleum and dried. 

Sodium perborate tetrahydrate (PBS-4) has been shown to oxidize a wide range of aromatic aldehydes to acids in excellent yield under mild conditions in acetic acid solvent (Figure 3.48).231... 

Inorganic peroxygens have also been used to oxidize sulfur centres, particularly sodium perborate, which is excellent for oxidizing electron-deficient sulfides to sulfones.412 Sodium perborate tetrahydrate has been used to stereo-specifically oxidize a-methylbenzylamine thiols in acetic acid.413 The use of organic peracids such as MCPBA was not found to be stereospecific for the above mentioned oxidation. 

Sodium perborate tetrahydrate was purchased from Aldrich Chemical Company, Inc. and used as received. 

Derivation By partial dehydration of sodium perborate tetrahydrate. 

---