Solid hypochlorites, decomposition

Solid Sta.te. The stabiHty of neutral calcium hypochlorite is primarily a function of moisture, lime, impurities, and temperature. Product containing - 7% water may lose 2—3% av CI2 during the first year when stored in warehouses without temperature control in moderate climates. Decomposition produces CaCl2, Ca(C102)2, and O2. 

D/chloro-5-Cyclohexyl-2-Oxo-2,3-D/hydro 1 H-Benzo(fj-Diazepine-1,4 fa) Process Using Sodium Hypochlorite — 40 ml of a solution of sodium hypochlorite of 14.5 British chloro-metric degrees are added to a suspension of 5.4 grams of 7 chloro-5 cyclohexyl-2 oxo-2,3-dihydro 1 H-benzo(f)diazepine-1,4 in BO ml of methylene chloride. The mixture is stirred at room temperature for 15 minutes the solid dissolves rapidly. The organic iayer is decanted, washed with water, dried over anhydrous Sodium sulfate and the solvent evaporated under reduced pressure without exceeding a temperature of 30 C. The residue is taken up in a little diisopropyl ether and the crystals which form are dried. They are recrystallized as rapidly as possible from ethyl acetate. Colorless crystals are obtained (3.9 grams yield, B5%) MP < = 163°C, with decomposition. 

Sodium hypochlorite is usually sold in solution in water, where it makes a greenish-yellow liquid. (It is too hygroscopic—it absorbs water from the air—to be used conveniently in solid form.) Household bleaches usually contain sodium hypochlorite in a 3 percent to 6 percent solution. Some sodium hydroxide (lye) is added to keep the pH high to avoid decomposition. If the solution is made more acidic, sodium hypochlorite will dissociate, producing chlorine gas and oxygen. 

Although solutions of sodium hypochlorite are useful oxidizing agents, the solid is not very stable. Calcium hypochlorite is used in bleaches, swimming pool treatments, and so forth. The decomposition of OC1- is catalyzed by compounds containing transition metals. 

Small Quantities (White Phosphorus). Wear nitrile rubber gloves, laboratory coat, and eye protection. Work in the fume hood. Five g (0.16 mol) of white phosphorus are cut under water into 5mm pellets. The pellets are added to 800 mL (0.8 mol) of 1 M cupric sulfate (127.7 g or 199.7 g of CuS04 or CuS04-5H20, respectively, dissolved in 800 mL of water) solution in a 2-L beaker. The mixture is allowed to stand for about a week with occasional stirring. The phosphorus grad-ually disappears, and a fine black precipitate of copper and copper phosphide is formed. The reaction is complete when no waxy white phosphorus is observed when one of the pellets is cut under water. The precipitate is separated, and while still wet, transferred to 500 mL of laundry bleach (5% sodium hypochlorite), and then stirred for about 1 hour to ensure complete decomposition of copper phosphide. The solids are separated and packaged for disposal. The aqueous solution is washed into the drain.33... 

AMMONIUM PHOSPHATE or sec-AMMONIUM PHOSPHATE or AMMONIUM PHOSPHATE, DIBASIC or AMMONIUM PHOSPHATE, MONOBASIC (7783-28-0, dibasic 7722-76-1,monobasic) HgN04P (monobasic) H9N2O4P (dibasic) Noncombustible solid. Contact with air slowly forms anhydrous ammonia. Contact with caustics forms anhydrous ammonia gas. Violent reaction with strong oxidizers, potassium chlorate sodium hypochlorite strong bases. Reacts with antimony(V) pentafluoride lead diacetate magnesium, silver nitrate zinc acetate. Heat of decomposition produces toxic fiimes of ammonia and phosphorus oxides. 

BIS (AMMONIUM) CARBONATE (506-87-6) (NH4)2COj Slightly combustible solid (Fire Rating 1). Contact with sodium hypochlorite causes sudden, possibly violent, decomposition. Becomes unstable and decomposes on exposure to air or in heat with loss of ammoiua and carbon dioxide, converting to powdery-white ammonium bicarbonate. Inconpatible with acids, acid salts, alkaloids, aluminum, calomel, iron salts, sodium nitrate, nitrites, zinc. Attacks nickel, copper, and other alloys. 

NICKEL CYANIDE or NICKEL CYANIDE, SOLID or NICKEL(II) CYANIDE (557-19-7) Ni(CN), A thermally unstable solid. Violentreaction with fluorine, hypochlorites, nitric acid, nitrates, nitrites, magnesium + heat. Contact with acids or heat releases deadly hydrogen cyanide gas. Incompatible with sulfur, selenium, active metals, sulfur, selenium. Explosive reaction with chlorates, nitrates, and other materials in heat above 842°F/450°C. Thermal decomposition releases toxic cyanide fumes. On small fires, use dry chemical powder (such as Purple-K-Powder), foam, or COj extinguishers. 

OXALIC ACID (144-62-7) CjHjO. HOOCCOOH Combustible solid heat-sensitive. (combustible <215 F/101°C. Fire Rating 1). Exposure to elevated temperatures, hot surfaces, or flames causes decomposition and the formation of toxic and flammable formic acid and carbon monoxide. Hygroscopic the solution in water is a medium-strong acid. Violent reaction with strong oxidizers, acid chlorides alkali metals bromine, furfuryl alcohol hydrogen peroxide (90%) phosphorus trichloride silver powders sodium, sodium chlorite sodium hypochlorite urea + heat (forms NHj gas, CO2 and CO may explode). Mixture with some silver compounds forms explosive salts of silver oxalate. Incompatible with caustics, mercury, urea. On small fires, use dry chemical powder (such as Purple-K-... 

EXPLOSION and FIRE CONCERNS noncombustible solid not expected to be a fire hazard forms an explosive product when reacted with carbon monoxide reacts violently with hydrogen peroxide violent reaction with aluminum calcium hypochlorite, and ethylene oxide no infoimation found concerning hazardous decomposition products in case of fire in surroundings, use carbon dioxide or dry chemical for firefighting purposes. 

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