Carbonate minerals alkali

If solid samples are insoluble in water, some decomposition procedure must be used. For inorganic materials, decomposition with mineral acids is most often employed (for a survey of decomposition techniques see [33]). When the sample cannot be dissolved in an acid, it can either be fused (most often with alkali carbonates, hydroxides or their mixtures [157, 47]) or sintered (usually with mixtures of alkali carbonates with divalent metal oxides, sometimes in the presence of oxidants [54]). Sintering is usually preferable, because then contamination of the sample and the resultant ionic strength are lower than is the... 

Carbonatites. Carbonatites are igneous mixtures of essentially carbonate minerals found in the form of intrusions and lavas, associated with highly undersaturated alkali igneous complexes along major rift zones, cutting old stable continental shield areas. 

Reactions with alkali feldspars do not provide divalent cations for the precipitation of carbonate minerals and initially were thought to be of little significance for mineral trapping (Gunter et al. 1997). However, more recent work indicates that dissolution of alkali feldspars contributes to the fixing of C02 as the sodium alumino-carbonate mineral dawsonite, NaAlC03(0H)2 (Johnson et al. 2001). In this case, the Na necessary for dawsonite precipitation is available in abundance in the brine, but dissolution of alkali feldspar provides a source of aluminum and neutralizes the acidic C02 according to (Johnson et al. 2001) ... 

If iron is present, the dry residue is subjected for several weeks to sunlight which renders the iron insoluble in acetic acid, after which acetic acid dissolves the calcium and magnesium carbonates which are separated by dilute sulphuric acid, precipitating calcium and dissolving magnesia. The residue from acetic acid treatment consists of clay, silicious matter and iron. The clay and iron are dissolved by marine acid (hydrochloric) and the iron precipitated by caustic alkali (phlogisticated alkali) and the clay by alkali carbonate. The silicious matter may be identified by its complete solution with effervescence under the blowpipe with mineral alkali (sodium carbonate). 

Zirconium oxide, Zr02 is widely known, both as a mineral, baddeleyite, and as an industrial product obtained horn zircon, Z1SO4. Moreover, the precipitate obtained by action of alkali hydroxides upon solutions of tetravalent zirconium is a hydrated oxide. The latter is readily soluble in acids to form oxysalts, which arc usually formulated in terms of the Zr02+ ion, without including its water of hydration, e.g., as Zr0(H2P04)2. The hydrated Zr02+ ion is not amphiprotic it does not dissolve in alkali hydroxides, While it does react on alkali carbonate fusions, the compounds formed have been shown to be mixed oxides rather than zirconates. 

The resulting Soln. C is a predominantly NaCl solution similar to terrestrial seawater (Soln. D, Table 5.3). Had we chosen a concentration factor of 600-fold, the agreement would have been even better. In any case, the concentration factor is arbitrary. The point is that simple processes, starting with a dilute Fe-Mg-HC03-rich solution formed by reaction of water with ultra-mafic and mafic rocks, evaporation, and carbonate precipitation, converted the solution into an Earth-like seawater NaCl brine. The Na/Mg ratio of solution C is 9.9, while terrestrial seawater has a Na/Mg ratio of 8.8 (Soln. 5.3D). Note also the similar pH values (8.03 and 8.05, Table 5.3). This solution did not (cannot) evolve into an alkali soda-lake composition as some have hypothesized or assumed for Mars (e.g., Kempe and Kazmierczak 1997 Morse and Marion 1999) because the mass of hypothesized soluble iron and magnesium and the low solubility of their respective carbonate minerals are sufficient to precipitate most of the initial soluble bicarbonate/carbonate ions. 

Alkali (monovalent) carbonate minerals also can occur in sediments. These phases have been studied in association with lake sediments. Their formation in these lacustrine environments has been used to deduce the conditions under which they formed based on their phase relations (see Figure 2.5). These phases usually precipitate during the late stages of evaporation of saline waters. 

Salts in addition to those of the Hand include our old friend Salt of Tartar, and the related sodium carbonate or Natron both used extensively in glass and ceramic glazes for their relative ease of fusion (about 900°C) and ability to dissolve many mineral bodies. These are often referred to as the Alkali Carbonates or just Alkali. 

The influence of amino and carboxylic groups on each other, when they are present in the same molecule, is quite small. Anthranilic acid dissolves as easily in carbonate solution as does benzoic acid, and as easily in aqueous hydrochloric acid as does aniline. Hence, an excess of either alkali or mineral acid must carefully be avoided if it is desired to isolate an aminocarboxylic acid in the free state. On the other hand, a slight excess of acetic acid does no harm. 

The mineral acids dissolve the crystals completely. When ignited in air, ferric oxide is obtained, as also when the crystals are fused with an alkali carbonate. Double salts formed by union with the fluorides of the alkali and certain other metals have been described.3 These may be termed... 

Soluble 1 in 300 of water practically insoluble in ethanol, chloroform, and ether soluble in aqueous solutions of mineral acids and alkali carbonates. 

Uranyl Carbonate occurs in a fairly pure condition in the mineral rutherfordine (see p. 273). It has not been obtained artificially. The addition of an alkali carbonate to solutions of uranyl salts yields precipitates of var nng conqiosition consisting of basic carbonates sometimes mixed vnth uranate. ... 

The previous arsinic acid in hydrochloric acid solution containing a little potassium iodide is saturated at 10 C. with sulphur dioxide and the gM passed for one hour. The addition of an equal volume of hydrochloric acid then precipitates 3-hydroxy-l 4-benzisoxazine-6-dichloro-arsine in 60 per cent, yield, but the product is difficult to purify. Solution in 2N sodium hy oxide and addition of hydrochloric add until only a faint acidity is shown to (Jongo red, causes the arsenoxide to separate in sphsero crystals, insoluble in water, dilute mineral acids, alkali carbonates, or dilute ammonia, but readily soluble in an excess of dilute caustic alkali solution. Treatment with excess of hydrochloric acid gives the dichloroarsine. 

The chemical name for potash is potassium carbonate (K2CO3). Early humans also knew about a similar substance called mineral alkali. This material was made from certain kinds of rocks. But it also had alkali properties. Mineral alkali was also called soda ash. The modern chemical name for soda ash is sodium carbonate (Na2C03). 

Manganese(ll) carbonate occurs naturally as the mineral rhodochrosite. It is manufactured from manganese(ll) sulfate by precipitation with alkali carbonates, or alkali or ammonium hydrogen carbonate ... 

The alkali-bearing minerals found in the blast furnace include kalio-philite-nepheline, leucite, plagioclase, and alkali carbonates [40-44], Kaliophilite was the dominant reaction product on the inside surface of the lining and in the joints between brick. The formation of this compound is accompanied by about a 45% volume increase. No kaliophilite, however, formed in the interior of the brick except in the carbon-disintegration zones. 

Van Vlack [42] observed that the bosh region contained alkalies in excess of the requirements of kaliophilite and nepheline. This excess did not result in the formation of alumino-silicate or silicate minerals of higher alkali content but was present as alkali carbonates. The carbonates formed toward the end of the furnace campaign from the free alkali deposited in the bosh lining. For the particular furnace examined, Van Vlack determined that alkali-bearing minerals were present only where porosity and proximity of the surface permitted expansion. Therefore, the presence of alkalies did not prove seriously detrimental in the bosh and... 

Formaldoxime has been applied in the determination of manganese in water [69,70], plants [69,71], silicate and carbonate minerals [72], uranium oxide [9], tin [73], and alkalies [74]. The formaldoxime method has been automated in the determination of manganese in water [75] and in silicate minerals [76]. The FIA technique has been applied in the analysis of natural waters [77] and silicates [78]. 

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