Salts calcium, solubility, table

As examples of some water-soluble salts, mention may be made of potassium chloride, copper sulfate, and sodium vanadate. As examples of some water-insoluble salts, mention may be made of some typical ones such as lead chloride, silver chloride, lead sulfate, and calcium sulfate. The solubilities of most salts increases with increasing temperature. Some salts possess solubilities that vary very little with temperature or even decline. An interesting example is provided by ferrous sulfate, the water solubility of which increases as temperature is raised from room temperature, remains fairly constant between 57 and 67 °C, and decreases at higher temperatures to below 12 g l-1 at 120 °C. Table 5.2 presents the different types of dissolution reactions in aqueous solutions, and Table 5.3 in an indicative way presents the wide and varied types of raw materials that different leaching systems treat. It will be relevant to have a look at Table 5.4 which captures some of the essential and desirable features for a successful leaching system. 

Barium is a member of the alkaline-earth group of elements in Group 2 (IIA) of the period table. Calcium [7440-70-2], Ca, strontium [7440-24-6], Sr, and barium form a closely allied series in which the chemical and physical properties of the elements and their compounds vary systematically with increasing size, the ionic and electropositive nature being greatest for barium (see Calcium and calcium alloys Calcium compounds Strontium and STRONTIUM COMPOUNDS). As size increases, hydration tendencies of the crystalline salts increase solubilities of sulfates, nitrates, chlorides, etc, decrease (except fluorides) solubilities of halides in ethanol decrease thermal stabilities of carbonates, nitrates, and peroxides increase and the rates of reaction of the metals with hydrogen increase. 

The type and concentration of the acid(s) can have a marked effect on the neutralisation process, largely owing to the solubility of the reaction product(s). The acids most commonly found in waste water are nitric (HNO3), hydrochloric (HCl), sulfuric (H2SO4), hydrofluoric (HF) and phosphoric (H3PO4). The solubilities of their calcium and magnesium salts are summarised in Table 28.6 [28.7] (N.B., all sodium salts are soluble). 

Anions are another factor controlling the stoichiometric efficiency of organic acids. In the case where carbonic acid acts as a solvent for carbonate cement the carbonate ions in solution result from the solvent (acid) as well as from the mineral dissolved. In contrast to this, for acetic acid as the solvent, at least half of the carbonate ions produced during dissolution will be substituted by acetate anions calcium acetate and not merely calcium carbonate alone is also a product of the dissolution. Calcium acetate is three times more soluble in water than calcium carbonate (Table 4.5). This actually favours the stay of the calcium ions in solution, hindering their precipitation in the form of calcium carbonate. Thus, the higher solubility of the salts of a... 

Although many sulfate salts are soluble in water, calcium sulfate is not (Table 7.1). Therefore, a solution of calcium chloride will react with sodium sulfate solution to produce a precipitate of calcium sulfate. The balanced equation is... 

Several compounds of the CaO—P2O3—H2O system are given in Table 8. The common names for the mono-, di-, and tricalcium phosphates arise from the traditional double-oxide formulas, CaO 2i5p T2O3, 2CaO H2O +205, and 3CaO +205, respectively. These terms are routinely used in industry. With the exception of the monocalcium salt, the calcium phosphates are all sparingly soluble. 

Since commercial products are mixtures of homologs they are more soluble than the pure components due to the solubilizing effect of the short-chain homologs as mentioned above. Table 5 shows the solubility in water of calcium salts of alcohol sulfates at 25°C [73]. 

On the other hand, remineralisation may occur at such a rate that the surface layer is retained (Table 2). This requires continuous renewal of ions, either from among those newly solubilised or from those present anyway in the saliva. This process has been discussed in terms of thermodynamics, in particular of the solubilities of the various possible calcium phosphate salts [34]. The present authors are wary of this approach, as what is involved is essentially a kinetic... 

Table 2 The solubility of ChLM Disks and Precipitation of Calcium salts.

C. Sulfamates prepared from weak bases form acidic solutions, whereas those prepared from strong bases produce neutral solutions. The pH of 5 wt % solution of ammonium sulfamate is 5.2. Crystals of ammonium sulfamate deliquesce at relative humidity of 70% and higher. Both ammonium sulfamate [7773-06-0] and potassium sulfamate [13823-30-2] hbemte ammonia at elevated temperatures and form the corresponding imidodisulfonate (12). Inorganic sulfamates are quite water-soluble, except for the basic mercury salt. Some relative solubilities of sulfamates at 25°C in 100 g of water are ammonium, 103 g sodium, 106 g magnesium, 119 g calcium, 67 g barium, 34.2 g zinc, 115 g and lead, 218 g. The properties of a number of sulfamates may be found in the literature (see Table 5). 

Various milk salts are interrelated and the interrelationships are affected by pH (Table 5.3). Those constituents, the concentrations of which are related to pH in the same way, are also directly related to each other (e.g. the concentrations of total soluble calcium and ionized calcium), while those related to pH in opposite ways are inversely related (e.g. the concentrations of potassium and sodium). 

The partition of salts between the soluble and colloidal phases is summarized in Table 5.5. In general, most or all of the sodium, potassium, chloride and citrate, one-third of the calcium and two-thirds of the magnesium and about 40% of the inorganic phosphate are in the soluble phase. 

In this study, the solubilities of carbon dioxide were represented by the Bunsen absorption coefficients and their values given in Table I for lithium chloride and in Table II for calcium chloride. The densities of salt solutions are... 

CALCIUM CHLORIDE. Calcium chloride. [CAS I004.7-52-4J. CaClj, is a white, crystalline salt that is very soluble in water. Solutions containing 30-45 wl % CaCh are used commercially. Of the alkaline-earth chlorides it is the most soluble in water, h is extremely hygroscopic and liberates large amounts of heat during water absorption and on dissolution. It forms a series of hydrates containing one. two, four, and six moles of water per mole of caJcium chloride (Table I). Another hydrate. CaCl 0.331 I O. has been identified, mol wi 116.98 94.8 wl % CaCl, heat of solution in water to infinite dilution. -71.37 kJ/mol (- 17.06 keal/mol). 

Trivalent chromium compounds, with the exception of acetate, hexahydrate of chloride, and nitrate salts, are generally insoluble in water (Table 3-2). Some hexavalent compounds, such as chromium(VI) oxide (or chromic acid), and the ammonium and alkali metal salts (e.g., sodium and potassium) of chromic acid are readily soluble in water. The alkaline metal salts (e.g., calcium, strontium) of chromic acid are less soluble in water. The zinc and lead salts of chromic acid are practically insoluble in cold water (Table 3-2). The hexavalent chromium compounds are reduced to the trivalent form in the presence of oxidizable organic matter. However, in natural waters where there is a low concentration of reducing materials, hexavalent chromium compounds are more stable (EPA 1984a). 

A major chemical plant dissolved inorganic slurry solids in a series of three fiberglass vessels. Most employees considered this section of the plant as one of the nonhazardous areas of this chemical complex. This area handled a relatively cool sodium chloride (table salt) water stream that was saturated with insoluble salts such as calcium carbonate and magnesium carbonate. The slurry contained about 30-percent calcium carbonate. Insoluble carbonates are treated with hydrochloric acid in two agitated vessels to allow a reaction to liberate carbon dioxide and form a soluble salt. The reaction is a simple one ... 

Information regarding the physical and chemical properties of the selected dinitrocresols is located in Table 3-2. Like dinitrophenols, the dinitrocresols are pseudoacids and readily form water soluble sodium, potassium, ammonium, and calcium salts (HSDB 1994 Metcalf 1978). Of the theoretically possible 18 isomers of dinitrocresols (Harvey 1953), the isomer 4,6-dinitro-o-cresol is the most commercially important (HSDB 1994). At a pH of 4.4, 50% of the DNOC in water exists as the dissociated compound (see pKa value in Table 3-2). The concentration of the ionized form increases as the pH increases. Essentially, 100% of the DNOC at pH 7 or above will be in the ionized form. Thus, in a whole animal all of the DNOC exists in the ionized form or is associated with a macromolecule such as albumin (King and Harvey 1953b). 

The ash content of soybeans is relatively high, close to 5 percent. The ash and major mineral levels in soybeans are listed in Table 5-7. Potassium and phosphorus are the elements present in greatest abundance. About 70 to 80 percent of the phosphorus in soybeans is present in the form of phytic acid, the phosphoric acid ester of inositol (Figure 5-5). Phytin is the calcium-magnesium-potassium salt of inositol hexaphosphoric acid or phytic acid. The phytates are important because of their effect on protein solubility and because they may interfere with absorption of calcium from the diet. Phytic acid is present in many foods of plant origin. 

The range of anions that can occupy the X positions is very wide (A11,D20) even anions that form calcium salts of very low solubility, such as ffuoride, can be introduced using special techniques. We shall consider only those most relevant to cement chemistry. Tables 6.2 and 6.3 include data. C3A CaCl2 l0H2O or [Ca2Al(0H)g]Cl-2H20 (Friedel s salt) can be formed in concrete exposed to chloride solutions. Two polytypes are known p is the... 

The solubility data of carbon dioxide in aqueous solutions of binary mixed salts obtained in this study are summarized in Table I those for ternary mixed salts are summarized in Tables II, III, and IV. Figures 1 and 2 show the solubility data for the potassium chloride-calcium chloride and sodium chloride-sodium sulfate-ammonium chloride mixed solutions, respectively, which are representative of all the data. The salting-out effect was shown in all the systems studied. 

Table III. Experimental Results of Carbon Dioxide Solubility in Aqueous Solutions of Potassium Chloride (1)—Sodium Chloride (2)—Calcium Chloride (3) Mixed Salt at 25°C and 1 atm...

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