Aluminum perchlorate

The first reported synthesis of acrylonitrile [107-13-1] (qv) and polyacrylonitrile [25014-41-9] (PAN) was in 1894. The polymer received Htde attention for a number of years, until shortly before World War II, because there were no known solvents and the polymer decomposes before reaching its melting point. The first breakthrough in developing solvents for PAN occurred at I. G. Farbenindustrie where fibers made from the polymer were dissolved in aqueous solutions of quaternary ammonium compounds, such as ben2ylpyridinium chloride, or of metal salts, such as lithium bromide, sodium thiocyanate, and aluminum perchlorate. Early interest in acrylonitrile polymers (qv), however, was based primarily on its use in synthetic mbber (see Elastomers, synthetic). 

Group 13 (IIIA) Perchlorates. Perchlorate compounds of boron and aluminum are known. Boron perchlorates occur as double salts with alkah metal perchlorates, eg, cesium boron tetraperchlorate [33152-95-3] Cs(B(C104)4) (51). Aluminum perchlorate [14452-95-3] A1(C104)2, forms a series of hydrates having 3, 6, 9, or 15 moles of water per mole of compound. The anhydrous salt is prepared from the trihydrate by drying under reduced pressure at 145—155°C over P2O5 (32). 

See also Alumina hydroxides classification, 2 422 Aluminum particle size, 10 22-23 Aluminum perchlorate, 18 278 Aluminum phosphide, 2 284 19 58 Aluminum-polyphenylenevinylene-ITO, in photovoltaic devices, 22 221 Aluminum production, 9 639-640 Aluminum recycling, 2 305 21 371-372 economic aspects of, 21 402 remelting, 2 333-334 Aluminum reduction, of ferrovanadium, 25 518... 

Aluminum Perchlorate. See under Perchlorates Aluminum Picrote. See under Picrates Aluminum Plate Test far Detonators is briefly described under Plate Tests and also in... 

Group 73 (IIIA) Perchlorates. Perchlorate compounds of boron and aluminum are known. Boron perchlorates occur as double salts with alkali metal perchlorates. Aluminum perchlorate, (CAS 14452-95-3J. Ai(C104)3. forms a series of hydrates. 

Aluminum perchlorate, A1(C104)3, is synthesized by treatment of AICI3 with AgC104 in CeHe (equation 30). It is a very strong oxidant that reacts slowly with paraffin hydrocarbons. It decomposes at 150 °C and should be considered a potential explosive. Aluminum periodate may be obtained in the same manner. Aluminum iodate, A1(I03)3, is obtained by thermal decomposition of [Al(0H2)6][I03][Hl206] HI03 at340°C. 

The anhydrous tris-chelate complexes of aluminum perchlorate are stable beyond 300°C (669). Trialkylaluminums form colored complexes with bipyridyl and phenanthroline (109) which are five-coordinate monomers (681). 

AICI3H18021 aluminum perchlorate nonahydrate 81029-06-3 25.00 2.0000 1 425 BaBr2H402 barium bromide dihydrate 7791-28-8 25.00 3.7000 1... 

Brosset (2), from measurements of the pH of aluminum perchlorate solutions, postulated that the product of hydrolysis of the aluminum ion is an infinite series of polynuclear complexes with the generalized formula Al[(OH)3Al]n3 Brosset, Biedermann, and Sillen (3) later recalculated Brosset s data and concluded that the major hydrolysis product could be either a single complex such as A16(OH)i53+ or an infinite series of complexes of the type Al[(OH)5Alo]n+3+w- Aveston, using ultracentrifugation, found evidence for either [Al2(OH)2]4+ or [Ali3(OH)32]7+. The latter species has been favored recently by Sillen (25) and by Johansson (26). 

If aluminum perchlorate solutions are made up to contain 4.54 X 10 4 moles/liter aluminum (total ionic strength about 10"2 molar), provided the nominal ratio of OHbo ndifferent types of aluminum which can be designated as AP, AP, and AP. A1 appears to be composed en-... 

From the titration and analysis data, the concentrations of Ala, Alb, and Ale can be calculated for any specific time. The concentrations of OH over and above the amount used in reacting with free H in the aluminum perchlorate titrant solution can be apportioned among these aluminum species by assuming that 1) Ala consists of Al AlOH Al(OH)2, and Al(OH)4, all of which are at equilibrium with one another at the pH of the solution in the reactor 2) Ah is Al(OH)3c, hence OHc is three times the determined value of Ale and 3) the remaining OH is combined with Alb. 

The rate of OH addition taken from the recorder trace of the pH-stat must first be adjusted to account for the free H that is added with the aluminum perchlorate solution. A further adjustment is required for the OH taken up by monomeric Ala species, assuming all these species are at equilibrium, controlled by the titration pH. 

The initial solutions contained aluminum perchlorate at concentrations of 10" or 10" M. They were maintained at constant total aluminum concentration and at an ionic strength of 0.01, and dilute sodium hydroxide was added slowly to each to attain the desired value of bound OH. The solutions were then aged in a C02-free atmosphere at 25°C. in polyethylene bottles. 

Aluminum metal reacts with perchloric acid to produce hydrogen gas and a solution of aluminum perchlorate. Write the molecular equation for this reaction. Then write the corresponding net ionic equation. 

Molecular sieves are used to remove water from hydrated salts or aqua-complexes. For example, [Mn(MeCN)6][C104]2 and [Fe(MeCN)6l[C104]2 are prepared from the corresponding aqua-complexes using molecular sieves.51/52 when zeolites are used in such dehydration processes, the reaction may proceed only slowly. Thus, hydrated aluminum perchlorate is transformed into [Al(Me0H)6][C104]3 using a zeolite in methanoP but the reaction takes six days. 

The propellant looks and feels like the hard rubber of a typewriter eraser. It is a mixture of aluminum powder as fuel, aluminum perchlorate powder as an oxidizer, a dash of iron oxide as a catalyst to speed the burning rate, and a polymer binder that also served as a fuel. It is not sensitive to ignition by static, friction, or impact and it will not detonate during storage. 

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