Source of sodium

Sodium is a common contaminant found in many chemicals. Reagent grade KCI, for example, may contain 40-50 ppm sodium. This is a significant source of sodium, given that its concentration in the salt substitute is about 100 ppm. 

G. D. Dub, Owens l ke—Source of Sodium Minerals Technical Publication No. 2235, American Institute of Mining and Metallurgical Engiueers, Sept. 1947. 

Additionally, it is a source of sodium oxide and a fluidizing agent. The amount of sodium nitrate added in the glass manufacture process is up to 2 wt % of the total raw material. 

Occurrence. The brines of Seades Lake, California are the sole brine source of sodium carbonate [497-19-8] (soda ash) production in the United States. There is a large underground deposit of sodium carbonate brine in the Sua Pan area of Botswana, Afdca (66). Another potential source is Owens Lake, California. Owens Lake brines were used to produce soda ash but were discontinued in 1967. 

Other sources of sodium ion that are used to make sodium citrate are sodium carbonate and sodium bicarbonate. These reactions evolve large volumes of carbon dioxide gas, resulting in much foaming but less exotherm. 

Less than half as much energy is needed to recover sodium carbonate from ores as it is to make it synthetically. The enviromnental impact is also less. However, because there is a limited distribution of natural soda ash in the world compared to the wide availability of salt and limestone, synthesis will continue to be a source of sodium carbonate outside the U.S. 

This chapter reviews recent experimental evidence of a bacterial source of sodium channel blockers, principly TTXs. These findings support the hypothesis that procaryotic organisms produce TTXs which contaminate oceanic food chains. 

The yellow color imparted to a natural gas flame originates from the ignition of sodium atoms or ions. The common source of sodium is salt (sodium chlo-... 

Although the Solvay process is still in use in some parts of the world, the chief source of sodium carbonate is the mineral trona, Na2C03 NaHC03 2H20. 

Some of the important compounds containing the group IA and IIA metals are the carbonates, nitrates, sulfates, and phosphates. We have already mentioned the mineral trona as the source of sodium carbonate. Calcium carbonate is found in many forms that include chalk, calcite, aragonite, and marble, as well as in egg shells, coral, and seashells. In addition to its use as a building material, calcium phosphate is converted into fertilizers in enormous quantities (see Chapter 14). 

Hypernatremia and fluid retention commonly occur, necessitating restricting daily sodium intake to no more than 3 g. All sources of sodium, including antibiotics, need to be considered when calculating daily sodium intake. 

Sodium chloride is widely distributed in nature. Oceans are the vast source of sodium chloride. It occurs in seawater at an average concentration of 2.68 wt%. It also occurs in many inland saline waters and in salt deposits in sedimentary rocks, as the mineral hahte. 

As mentioned previously (p. 421) ammonium chloride and sodium nitrate in stoichiometric proportion has also been suggested, as an effective source of sodium ions which possess marked ability to inhibit methane explosions. 

Cobalt-iodized salt is often used as a source of sodium, chloride, iodine and cobalt. 

Elementary Na/S battery science The basic science of the Na/S cell is identical to that of the fuel cell. In both cases the essential is an electrolyte. On one side of the electrolyte membrane there is a source of sodium ions at a particular chemical potential, and on the other side a sink for the ions at a relatively lower chemical potential. The elements of the process are illustrated in Fig. 4.28. 

In the United States, the major source of sodium carbonate is the mineral trona, which has the formula Na2C03-NaHC03-2H20. The fact that sodium bicarbonate (NaHC03) is present is no surprise in view of the fact that the carbonate reacts with water and carbon dioxide to produce sodium bicarbonate ... 

Our synthetic routes to ZK4 were modifications of those described by Kerr (21). An amorphous, basic aluminosilicate gel containing tetramethylammonlum (TMA) Ion was heated at 100°C to promote formation of ZK4 crystals. Preparation of the gel Involved the vigorous mixing at room temperature of one component acting as a source of sodium and alumina, with another component acting as a source of TMA and silica. The alumina used was sodium... 

The end result of the Chapman mechanism, and of the modified Chapman processes as elucidated by later investigators" "" is that sodium and other metals (if Chapman-like mechanisms hold for the other metals) are abundant in atomic form. The kinetic studies show that molecular compounds are not present in large quantities above 85 km. Further work " showed that following the formation of dense atomic trails during the vaporization process, molecular recombination in the wake occurs to form smoke or dust that can then act as a delayed source of sodium (and other) atoms. It was then suggested that NaO reacts with atmospheric H2O to form gaseous NaOH, with the latter reacting with atmospheric CO2 in a three-body reaction to form NaHCOs" ... 

HALIDES Halogens Halite sodium, chlorine TABLE SALT, source of sodium for LYE, improves workability of molten GLASS... 

Sodium never occurs as a free element in nature. It is much too active. It always occurs as part of a compound. The most common source of sodium in Earth is halite. Halite is nearly pure sodium chloride (NaCl). It is also called rock salt. 

Sodium borate can be prepared from minerals such as borosodium calcite, pandermite, or tinkal these are natural sodium or calcium borates. Treatment of the mineral with sodium carbonate and sodium hydrogencarbonate yields the sodium borate decahydrate. In the USA, brine from salt lakes is also an important source of sodium borate. ... 

Shah U, Augsberger L. Multiple sources of sodium starch glycolate NF evaluation of functional equivalence and development of standard performance tests. Drug Dev Ind Pharm 2002 7(3) 345-359. 

Use Source of sodium compounds, especially the sodium carbonates. 

A shift to the processing of substantial alternate natural mineral sources of sodium carbonate in the U.S. has eliminated the calcium chloride disposal problems of the Solvay process for sodium carbonate production. Coupling this advantage to the much lower capital cost of a natural sodium carbonate plant has contributed to the shift away from synthetic sodium carbonate in the U.S. [13] (Table 7.3). Kenya is the only other country reported to be recovering natural sodium carbonate and was operating at 260,000 metric toimes in 2001 [19]. China, the second largest producer, and all other world producers still rely heavily on the ammonia-soda process [17, 24] (Table 7.4). 

An additional source of sodium carbonate occasionally used is via the carbonation of electrolytic sodium hydroxide as it is formed in the cell, or separately, later (e.g., [26]). The precipitated sodium hydrogen carbonate is calcined to obtain sodium carbonate in a maimer similar to the last step of the Solvay process (Eq. 7.15). 

The average Na+ content of the human body is 60 mEq/kg, of which 50% is in extracellular fluid, 40% is in bone, and 10% is intracellular. The chief dietary source of sodium is salt added in cooking. Excess sodium is largely excreted in the urine, although some is lost in perspiration. Gastrointestinal losses are small except in diarrhea. 

Sodium restriction is also a necessary intervention. A diet with 3 g of sodium per day is usually a reasonable place to start. Ingestion of too much sodium is a common reason diuretic therapy fails. Clinicians should be vigilant about sources of sodium. For example, 1 L of 0.9% NaCl yields 154 mEq of sodium, or 3.5 g. Sodium is usually restricted even in patients who are receiving RRT. In continuous and intermittent RRTs there usually is no worry about hyponatremia developing because these therapies will incorporate isonatremic (135 to 140 mEq/L of sodium) solutions as dialysate or ultrafiltrate replacement solutions. Serum sodium concentrations should be monitored daily. 

Fluid and electrolyte replacement should be initiated at the onset of diarrhea. (ORT generally is not required in healthy individuals flavored mineral water offers a good source of sodium and glucose. ° ) For symptom relief, loperamide (preferred because of its quicker onset and longer duration of relief relative to bismuth) should be taken (4 mg orally initially and then 2 mg with each subsequent loose stool to a maximum of 16 mg/day in patients without bloody diarrhea and discontinued if symptoms persist for over 48 hours). Other symptomatic... 

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