Peroxide, barium sodium

Potassium bichromate. Antimony sulfide Potassium permanganate. Powdered sugar Barium chlorate, Paraffln wax Potassium perchlorate. Cane sugar Sodium nitrate. Sulfur Sodium peroxide. Sulfur Sodium chlorite. Aluminum powder Magnesium chlorate. Aluminum powder Guanidine nitrate. Antimony powder Ammonium nitrate. Gasoline... 

Concentrated acid solutions of vanadium pentoxide are reduced to the tetravalent state by hydrogen peroxide, the peroxides of sodium, barium, magnesium, and by persulphates of potassium and ammonium.4 Acid solutions of vanadium pentoxide give rise to pervanadic acid with hydrogen peroxide. 

Give formulas of the peroxides of sodium and of barium. How do these substances react with cold dilute acids What is the formula of the peroxide of potassium Compare the action of the oxides Na20, K20, and BaO in water with that of the peroxides. What is the valence of the metal in each of the peroxides, and how do you account for the amount of oxygen over that contained in the oxide ... 

Na202 - Sodium peroxide Ba02 - Barium peroxide NaN03 - Sodium nitrate Ba (N03) 2 - Barium nitrate NH4HC03 - Ammonium bicarbonate Na2C03 - Sodium carbonate NaHC03 - Sodium bicarbonate... 

DIFLUOROETHENE or DIFLUORO-l,l-ETHENE (75-38-7) Flammable gas (flash point <—85°F/<—65°C). Violent reaction with oxidizers, barium, sodium, or potassium. Reacts with aluminum chloride. Incompatible with hydrogen chloride. May form explosive compounds with light metals and metallic azides. Capable of forming unstable peroxides may cause explosive polymerization. Undergoes thermal decomposition when exposed to flame or red-hot surfaces. May accumulate static electricity, and cause ignition of its vapors. The uninhibited monomer vapor may block vents and confined spaces by forming a solid polymer material. 

Peroxides (inorganic) should be handled carefully. When mixed with combustible materials, barium, sodium, and potassium peroxides form explosives that ignite easily. 

Hydroxylamine Barium oxide and peroxide, carbonyls, chlorine, copper(II) sulfate, dichromates, lead dioxide, phosphorus trichloride and pentachloride, permanganates, pyridine, sodium, zinc... 

Quantitatively, sulfur in a free or combined state is generally determined by oxidizing it to a soluble sulfate, by fusion with an alkaH carbonate if necessary, and precipitating it as insoluble barium sulfate. Oxidation can be effected with such agents as concentrated or fuming nitric acid, bromine, sodium peroxide, potassium nitrate, or potassium chlorate. Free sulfur is normally determined by solution in carbon disulfide, the latter being distilled from the extract. This method is not useful if the sample contains polymeric sulfur. 

Pilocarpine dissolves in dilute soda solution, and the rotation is thereby reduced, due to the formation of the sodium salt of pilocarpic acid, CiiHigOgNa, of which pilocarpine is the lactone. Amorphous barium and copper salts have been prepared. Pilocarpine in dilute sulphuric acid gives with hydrogen peroxide, followed by potassium dichromate, a bluish-violet colour soluble in benzene. For the identification of the alkaloid Wagenaar recommends precipitation with gold chloride solution. 

Determination of sulphite by oxidation to sulphate and precipitation as barium sulphate Discussion. Sulphites may be readily converted into sulphates by boiling with excess of bromine water, sodium hypochlorite, sodium hypobromite, or ammoniacal hydrogen peroxide (equal volumes of 20-volume hydrogen peroxide and 1 1 ammonia solution). The excess of the reagent is decomposed by boiling, the solution acidified with hydrochloric acid, precipitated with barium chloride solution, and the barium sulphate collected and weighed in the usual manner (Section 11.72). 

Violence of reaction depends on concentration of acid and scale and proportion of reactants. The following observations were made with additions to 2-3 drops of ca. 90% acid. Nickel powder, becomes violent mercury, colloidal silver and thallium powder readily cause explosions zinc powder causes a violent explosion immediately. Iron powder is ineffective alone, but a trace of manganese dioxide promotes deflagration. Barium peroxide, copper(I) oxide, impure chromium trioxide, iridium dioxide, lead dioxide, manganese dioxide and vanadium pentoxide all cause violent decomposition, sometimes accelerating to explosion. Lead(II) oxide, lead(II),(IV) oxide and sodium peroxide all cause an immediate violent explosion. 

Hydrogen sulfide is rapidly oxidised, and may ignite in contact with a range of metal oxides, including barium peroxide, chromium trioxide, copper oxide, lead dioxide, manganese dioxide, nickel oxide, silver(I) oxide, silver(II) oxide, sodium peroxide, and thallium(III) oxide. In the presence of air, contact with mixtures of calcium oxide or barium oxide with mercury oxide or nickel oxide may cause vivid incandescence or explosion. 

MRH Barium peroxide 3.85/tr., calcium hypochlorite 3.77/52, lead dioxide 1.92/64, potassium dichromate 3.85/tr., potassium permanganate 2.80/49, sodium hypochlorite 3.97/53... 

Hydroxylamine is a powerful reducant, particularly when anhydrous, and if exposed to air on a fibrous extended surface (filter paper) it rapidly heats by aerobic oxidation. It explodes in contact with air above 70°C [1]. Barium peroxide will ignite aqueous hydroxylamine, while the solid ignites in dry contact with barium oxide, barium peroxide, lead dioxide and potassium permanganate, but with chlorates, bromates and perchlorates only when moistened with sulfuric acid. Contact of the anhydrous base with potassium dichromate or sodium dichromate is violently explosive, but less so with ammonium dichromate or chromium trioxide. Ignition occurs in gaseous chlorine, and vigorous oxidation occurs with hypochlorites. 

Solid sodium peroxide causes immediate ignition in contact with gaseous hydrogen sulfide [1]. Barium peroxides and other peroxides behave similarly [2],... 

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