Beryllium acid solutions

Chemical Reactivity - Reactivity with Water Reacts vigorously as an exothermic reaction. Forms beryllium oxide and hydrochloric acid solution Reactivity with Common Materials Corrodes most metals in the presence of moisture. Flammable and explosive hydrogen gas may collect in confined spaces Stability During Transport Stable Neutralizing Agents for Acids and Caustics Flush with water and rinse with dilute solution of sodium bicarbonate or soda ash Polymerization Not pertinent Inhibitor of Polymerization Not pertinent. 

Beryllium is sometimes precipitated together with aluminium hydroxide, which it resembles in many respects. Separation from aluminium (and also from iron) may be effected by means of oxine. An acetic (ethanoic) acid solution containing ammonium acetate is used the aluminium and iron are precipitated as oxinates, and the beryllium in the filtrate is then precipitated with ammonia solution. Phosphate must be absent in the initial precipitation of beryllium and aluminium hydroxides. 

Procedure. Transfer the almost neutral sample solution of beryllium (containing 5 to 80jug of the element in a volume of about lOmL) to a 25 mL graduated flask, add 2.8 mL of 2.0M sodium hydroxide (or more if much aluminium is present), 5.0 mL of 0.64M boric acid solution, and 6.0 mL of the dye solution (see Note), dilute to the mark with distilled water, and mix well. Measure the transmittance at 520 nm, or with a green filter preferably using a 2 cm cell. 

Most orthosilicates reacted completely with poly(acrylic acid) solution an exception was andradite, CagFOg [SiOJg. Even so, the cements of gehlenite and hardystonite were very weak and affected by water. Only gadolinite and willemite formed cements of some strength which were unaffected by water, probably because one contained beryllium and iron and the other zinc. 

Investigations of the equilibria obtaining in solution have provided information concerning the stoichiometry and stability of the species formed when the beryllium ion is hydrolyzed. Although the identification of the minor species can never be regarded as definitive, there is little doubt that the principal species are Be2(OH)3+ and Be3(OH)3+ in acid solutions and Be(OH)3 and Be(OH)r in strongly basic solutions. Further support for these conclusions is provided by some crystal structures. The structure of [Be3(0H)3(H20)6]... 

Beryllium. Be metal is relatively unreactive at room temperature it does not react with water and steam even at red heat and it does not oxidize in air below 600°C. Powdered beryllium burns in air brilliantly on ignition forming BeO and Be3N2. It reacts with the halogens and dissolves easily in dilute aqueous acid solutions. It is passivated by cold concentrate HN03. The Be compounds, especially as dusts or smokes, are extremely toxic (possibly due to the ability of Be11 to displace Mg11 from Mg-activated enzymes). 

Insoluble silica residues are removed by filtration. The solution now contains beryllium, iron, yttrium, and the rare earths. The solution is treated with oxalic acid to precipitate yttrium and the rare earths. The precipitate is calcined at 800°C to form rare earth oxides. The oxide mixture is dissolved in an acid from which yttrium and the rare earths are separated by the ion-exchange as above. Caustic fusion may be carried out instead of acid digestion to open the ore. Under this condition sihca converts to sodium sihcate and is leached with water. The insoluble residue containing rare earths and yttrium is dissolved in an acid. The acid solution is fed to an ion exchange system for separating thuhum from other rare earths. 

Assay of beryllium metal and beryllium compounds is usually accomplished by titration. The sample is dissolved in sulfuric acid. Solution pH is adjusted to 8.5 using sodium hydroxide. The beryllium hydroxide precipitate is redissolved by addition of excess sodium fluoride. Liberated hydroxide is titrated with sulfuric acid. The beryllium content of the sample is calculated from the titration volume. Standards containing known beryllium concentrations must be analyzed along with the samples, as complexation of beryllium by fluoride is not quantitative. Titration rate and hold times are critical therefore use of an automatic titrator is recommended. Other fluoride-complexing elements such as aluminum, silicon, zirconium, hafnium, uranium, thorium, and rare earth elements must be absent, or must be corrected for if present in small amounts. Copper—beryllium and nickel—beryllium alloys can be analyzed by titration if the beryllium is first separated from copper, nickel, and cobalt by ammonium hydroxide precipitation (15,16). 

As with lithium, many properties of beryllium stand distinctly apart from those of its congeners. Again, the tiny size of the beryllium ion is responsible for the peculiarities. If we arbitrarily call the volume of the magnesium ion 1.0 unit, the volumes of the calcium, strontium, and barium ions become, respectively, about 3, 5, and 8 units however, the volume of the beryllium ion is, on the same scale, only 1/8 unit. Since the oxide is amphoteric, one would expect many of the salts of Be+2 to be extensively hydrolyzed in water (as is the case with the salts of Al8+, Zn2+, and Cr8+). The acidity of beryllium-containing solutions is also increased by polymerization of the beryllium-containing ions ... 

To 100 ml of sample 10 ml of 1M ammonium tartrate is added and the pH of the solution is adjusted to 6.0 0.5 by adding dilute ammonium hydroxide or tartaric acid solution as necessary. Transfer the solution to a 150 ml separatory funnel and add 10 ml of extractant solution. Shake for one minute then allow to stand for three to five minutes. Withdraw the organic layer and store in stoppered tubes prior to analysis. The APHA [8] use a similar extraction technique for the determination of beryllium and aluminium in water employing a nitrous oxide flame in the subsequent atomic absorption analysis, and using MIBK as a solvent. 

Iron interferes with the test and should be absent. Chromium forms a similar lake in acetate solution, but this is rapidly decomposed by the addition of the ammoniacal ammonium carbonate solution. Beryllium gives a lake similar to that formed by aluminium. Phosphates, when present in considerable quantity, prevent the formation of the lake. It is then best to precipitate the aluminium phosphate by the addition of ammonia solution the resultant precipitate is redissolved in dilute acid, and the test applied in the usual way. 

Cupferron reagent fiocculent yellow precipitate of the titanium salt, Ti(C6H502N2)4, in acid solution (distinction from aluminium and beryllium). If iron is present, it can be removed by precipitation with ammonia and ammonium sulphide solutions in the presence of a tartrate the titanium may then be precipitated from the acidified solution by cupferron. 

Oxalic acid solution white, crystalline precipitate of thorium oxalate, Th(C204)2 (distinction from aluminium and beryllium), insoluble in excess of the reagent and in 0-5m hydrochloric acid. 

Saturated potassium sulphate solution white, crystalline precipitate, having the composition Ce2(S04)3.3K2S04 in neutral solution and Ce2(S04)3. 2K2S04.2H20 from slightly acid solution (difference from aluminium and beryllium). 

Decrystallization of cellulose by swelling agents or solvents can be brought about by concentrated sodium hydroxide amines me-tallo-organic complexes of copper, cadmium, and iron quaternary ammonium bases concentrated mineral acids (sulfuric, hydrochloric, phosphoric) concentrated salt solutions (beryllium, calcium, lithium, zinc) and a number of recently investigated mixed solvents (J6). 

Beryllium may be separated by extraction with benzohydroxamic acid and some of its derivatives (including heterocyclic ones [6]), in cyclohexanone [7] and with Aliquat 336S in xylene from malonic acid solution (pH 5-7) [8,9]. Beryllium has also been extracted from thiocyanate media with TBP in toluene [10] and TOA in MIBK [11]. 

BERYLLIUM DIFLUORIDE or BERYLLIUM FLUORIDE (7787-49-7) BeFj Mixture with water form an acid solution. Incompatible with acids, caustics, chlorinated hydrocarbons, oxidizers, molten lithium, magnesium Aqueous solution is incompatible with organic anhydrides, acrylates, aleohols, aldehydes, alkylene oxides, substituted allyls, cresols, eaprolactam solution, epiehlorohydrin, ethylene dichloride, glycols, isocyanates, ketones, maleie anhydride, nitrates,... 

Very pure oxide may be obtained when the beryllium nitrate prepared as described above is reconverted to the carbonate. An acid solution of the nitrate is evaporated in a platinum dish to remove excess acid, the residue is dissolved in some water, and enough distilled ammonium carbonate solution is added to redissolve the initially precipitated beryllium carbonate andgive a clear solution. The solution is then evaporated in a platinum dish until all the beryllium carbonate has separated as a coarse precipitate. After thorough washing with pure water and then with freshly distilled alcohol, the product is dried and finally calcined to the oxide in a platinum vessel placed in an electric furnace at 900°C. 

Group 2 All react vigorously to produce ionic chlorides of formula MCI2, except that BeClj is covalent when anhydrous. All Group 2 chlorides are soluble in water producing hydrated ions of formula [M(H20)J L Beryllium chloride gives an acidic solution because of... 

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