Ferric acetates phosphate

Dioctyl Phosphate 3115-39-7 Ethoxyethyl Acetate (2-) 111-15-9 Ferric Acetate 1834-30-6... 

Benzal chloride is hydrolyzed to benzaldehyde under both acid and alkaline conditions. Typical conditions include reaction with steam in the presence of ferric chloride or a zinc phosphate catalyst (22) and reaction at 100°C with water containing an organic amine (23). Cinnamic acid in low yield is formed by heating benzal chloride and potassium acetate with an amine as catalyst (24). 

J. J. Berzelius prepared lead phosphate by adding a soln. of lead acetate to a nitric acid soln. of bone-ash, and decomposed the lead phosphate by treatment with dil. sulphuric acid, and removed the last traces of lead by hydrogen sulphide and W. Odling treated a soln. of sodium phosphate in ice-cold water with lead acetate, and decomposed the washed precipitate suspended in water with hydrogen sulphide. The soln., freed from the precipitated lead sulphide, was evaporated to remove the hydrogen sulphide. J. Persoz digested the soln. of bone-ash with ferric or aluminium oxide, decomposed the precipitated phosphate with sulphuric acid, and afterwards extracted with phosphoric acid with alcohol. L. Thompson precipitated the lime by treating the calcium phosphate with oxalic acid. W. H. Ross and co-workers purified phosphoric acid by a process of fractional crystallization. 

The precipitates obtained with magnesia mixture (magnesium chloride in ammoniacal solution), or ferric chloride in an acid solution to which sodium acetate has been added, are often used as tests for phosphate (see p. 180), and in the latter case the phosphate is removed from solution as ferric phosphate. Another common test is the formation of yellow ammonium phosphomolybdate when, a nitric acid solution of ammonium molybdate is added to phosphate solution (see pp. 180, 181). 

Ferric Phosphate occurs as a yellow-white to buff colored powder. It contains from one to four molecules of water of hydration. It is insoluble in water and in glacial acetic acid, but is soluble in mineral acids. 

The resulting salt, whilst readily soluble in dilute mineral acids, is insoluble in cold acetic acid, phosphoric acid, and sodium phosphate. It is slightly soluble in citric and tartaric acid solutions, and readily dissolves m neutral aqueous ammonium citrate, yielding a green solution with a brownish tint.3 The salt is insoluble in water, but hot water hydrolyses it, and boiling with excess of ammonia solution converts it into a mixture of ferric hydroxide 4 and ferric phosphate, or if the ammonia is present in great excess the ferric phosphate may be entirely decomposed. Thus —... 

SAFETY PROFILE Experimental poison by subcutaneous route. Moderately toxic to humans by ingestion. Moderately toxic experimentally by ingestion, intraperitoneal, and intravenous routes. An experimental teratogen. Human systemic effects by multiple and unspecified routes toxic psychosis, excitement, respiratory stimulation, nausea or vomiting, and sweating. Experimental reproductive effects. Mutation data reported. A powerful irritant which affects the central nervous system. Incompatible with ferric salts, mineral acids, iodine, lead acetate, silver nitrate, sodium phosphate powder. When heated to decomposition it emits toxic fumes of Na20. 

When these factors were taken into account, and velocities were determined at dilute concentrations of substrate and in the presence of 0.1 M acetate, pH 5.5, as buffer and 0.01 M EDTA, it was possible to determine the Michaelis constants for different substrates. At 37°C these values were as follows a-glycerophosphate, 3.1 mJlf j8-glycerophos-phate, 2.4 mM yeast adenylate, 0.25 mAf phenyl phosphate, 0.15 mAf. The corresponding values for Tmax, the velocity at infinite substrate concentration, were expressed as micrograms of phosphate liberated per minute 0.9, 1.0, 1.0, and 1.0. With phenyl phosphate as substrate, L-( + )-tartrate was found to be a strong competitive inhibitor, with Ki equal to 0.63 X 10" Af. The enzyme was also reversibly inactivated by cupric and ferric ions and by the thiol reagent, p-chlormercuribenzoate. 

CHLORURE PERRIQUE (French) (7705-08-0) Very hygroscopic contact with moisture in air forms ferric chloride hexahydrate. Aqueous solution is highly acidic, precipitating hydroxide and phosphate salts, and forming corrosive fumes. Violent reaction with strong bases, allyl chloride, bromine pentafluoride, ethylene oxide, oxygen difluoride. Shock- and friction-sensitive explosive is formed with potassium, sodium, potassium-sodium aUoy, and possibly with other active metals. Aqueous solution is incompatible with sulfuric acid, caustics, ammonia, aliphatic amines, alkanolamines, amides, organic anhydrides, isocyanates, vinyl acetate, alkylene oxides, epichlorohydrin. Attacks metals in the presence of moisture. 

Incompot Ferric salts, lime water, spirit nitrous ether, mineral acids, iodine, lead acetate, silver nitrate, sodium phosphate in powder. 

Electrolytes which do not afford ionic complexes with common hexitols and reducing sugars are aqueous solutions of lead acetate, copper sulfate, zinc sulfate, ferrous ammonium sulfate, calcium chloride, potassium dichromate, ferric chloride (pH 3), aluminum sulfate, magnesium sulfate, sodium sulfate, potassium antimonyl tartrate, sodium arsenate or arsenic acid, sodium phosphate, and hydrochloric acid. It is not certain whether sodium aluminate (in 0.1 N sodium hydroxide) affords ionic complexes with carbohydrates, as aqueous alkali, alone, permits their migration during electrophoresis. 

Phosphates.—Triferrous Phosphate—Fes(P04)3—857.7.—A white precipitate, formed by adding disodic phosphate to a solution of a ferrous salt, in presence of sodium acetate. By exposure to air it turns blue a part being converted into ferric phosphate. The ferri phosphas (Sr.) is such a mixture of the two salts. It is insoluble in HsO sparingly soluble in HsO containing carbonic or acetic acid. 

Ferric phosphate L-Lysine Nicotinic acid Retinyl acetate DL- rine nutrient, fermentation Methyl eicosanoate Methyl stearate ... 

In an orthophosphoric acid-dihydrogen phosphate buffer (130), the rate of the acidic decomposition of chlorous acid appears to be independent of the concentration of added ferric ion, whereas in an acetate buffer (167), ferric ion was found to catalyze the decomposition of chlorous acid, Nakamori et al. (167) reported that ferric ion, cupric ion, cobalt(II) ion, and nickel (II) ion change the stoichiometry and catalyze the rate of decomposition of chlorous acid at pH 3.5 in an acetate buffer. Their conclusions, however, are subject to question, since they used the chloride salts of the metals as catalysts. In view of the known effects of chloride ion on the stoichiometry... 

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