Potassium bicarbonate carbonate

Tosh, J. S., J. H. Field, H. E. Benson and W. P. Waynes, "Equilibrium Study of the System Potassium Carbonate, Potassium Bicarbonate, Carbon Dioxide and Water," U. S. Bureau of Mines, Report of Investigations, 1959, 5484. 

Subphase buffers at pH 9-11 and 0.1 to 0.2 ionic strength were prepared with sodium or potassium bicarbonate-carbonate mixtures (8, 26). Subphase buffers at pH 8-11 were prepared by adding 0.01M tris to 0.1M or 1.0M sodium chloride and adjusting the pH with concentrated hydrochloric acid or concentrated sodium hydroxide. Another alkaline subphase contained 0.1 N sodium hydroxide (pH 12.7). The acid subphase contained 0.01N hydrochloric acid and 0.1M sodium chloride (pH 2.1). All subphases contained 0.1mM EDTA. 

Carbonic acid monoammonium salt. See Ammonium bicarbonate Carbonic acid monopotassium salt. See Potassium bicarbonate Carbonic acid monosodium salt. See Sodium bicarbonate... 

A large amount of comprehensive physical data on the potassium carbonate-potassium bicarbonate-carbon dioxide-water and potassium carbonate-potassium bicarbonatepotassi-um bisulfide-carbon dioxide-hydrogen sulfide-water systems is available in literature (Benson et al., 1954 Benson et al., 1936 Tosh et al., 1959 Tosh et al., 1960 Allied Chemical Coip., 1961 Bocard and Mayland, 1962). Some typical data are given below however, fm complete information, the reader is referred to the original sources. 

Additional vapor-liquid equilibrium data based on published iitformation and ejqterimen-tal work have been reported by Bocard and Mayland (1962). Other physical data on the potassium carbonate-potassium bicarbonate-carbon dioxide system are shown in Figures 5-11 to 5-14. The data of Bocard and Mayland (1962) have been converted to a series of nomographs by Mapstone (1966). 

Benzenetetrol. 1,2,3,5-Tetrahydroxybenzene (64) forms needles (mp 165°C) from water. The compound is easily soluble ia water, alcohol, and ethyl acetate and is iasoluble ia chloroform and benzene. In aqueous potassium bicarbonate solution sparged with carbon dioxide,... 

Amino-2-hydroxybenzoic acid is manufactured by carboxylation of 3-amiaophenol under pressure with ammonium carbonate at 110 °C (182) or with potassium bicarbonate and carbon dioxide at 85—90°C (183) with subsequent acidification. 

A.ctivated Carbonate Process. The activated carbonate process is based on absorption of CO2 by potassium carbonate (57) to give potassium bicarbonate. When the bicarbonate is heated it releases CO2, regenerating potassium carbonate. 

Other bicarbonates of considerable commercial importance are ammonium bicarbonate [1066-33-7] and potassium bicarbonate [298-14-6]. These compounds are decomposed by the oven heat, Hberating ammonia, carbon dioxide, and water to faciUtate leavening action. Their uses are limited to low moisture products such as cookies and crackers. 

Potassium Carbonate Process. The potassium carbonate process is similar to the sodium carbonate process. However, as potassium bicarbonate [298-14-6] is more soluble than the corresponding sodium salt, this process permits a more efficient absorption than the other. The equipment layout is the same and the operation technique is similar. 

Partly because of their low cost, aqueous solutions of sodium or potassium carbonate also are used for CO9 and H9S. Potassium bicarbonate has the higher solubility so the potassium salt is preferred. In view of the many competitive amine and carbonate plants that are in operation, fairly close figuring apparently is required to find an economic superiority, but other intangibles may be involved. 

To the epoxide dissolved in a minimal amount of chloroform or ether is added a corresponding solution of freshly prepared thiocyanic acid (20 fold excess) as described above (acetic acid has also been used as solvent). The resulting solution is allowed to stand at least 70 hr at room temperature. (Some workers have protected the reaction mixture from light during this period). The reaction mixture is worked up by washing first with a 10% solution of sodium carbonate, sodium bicarbonate or potassium bicarbonate, and then water. The remaining ether extract is dried (Na2S04) and evaporated under vacuum. The crude thiocyanatohydrin is crystallized from an appropriate solvent or treated with methanesulfonyl chloride s (see below). 

Hydrolysis of the intermediate epoxy acetate is generally carried out with strong alkali if base-sensitive groups are present, milder conditions (e.g., potassium bicarbonate, potassium carbonate) can be employed. If commercial peracetic acid (which contains sulfuric acid) is used for epoxidation, the intermediate epoxy acetate cannot be isolated, but is hydrolyzed in situ by the acid to the desired ketol. Acid hydrolysis will also retain 3-acetates, if present. ... 

The solution concentration for a potassium carbonate system is limited by the solubility of the potassium bicarbonate (KHCO3) in the rich... 

Fig. 8. Preparative isolation of hexon antigen of EDS-76 by hydrophobic-interaction chromatography on Butyl-PG column (2x5 cm) (A) application of the allantoic fluid diluted (1 5) by 50 mM potassium acetate, pH 4,130 ml (B)0.01 mol/1 potassium acetate, pH 5.5 (C) 0.01 mol/1 potassium bicarbonate pH 8.0, 10% isopropanol (D) 0.01 mol/1 potassium carbonate pH 9.6, 10% isopropanol. EDS-0 — components of alantoic fluid eluted with buffer A, EDS-1 — desorbed hexon fraction eluted with buffer C, EDS-2 — fraction desorbed with buffer D [56]...

Carbonic anhydrase is an enzyme that produces free hydrogen ions, which are then exchanged for sodium ions in the kidney tubules. Carbonic anhydrase inhibitors inhibit the action of the enzyme carbonic anhydrase This effect results in the excretion of sodium, potassium, bicarbonate, and water. Carbonic anhydrase inhibitors also decrease the production of aqueous humor in the eye, which in turn decreases intraocular pressure (IOP) (ie, the pressure within the eye). 

The submitters state that the failure to add dry ice at this point may result in greatly reduced yields. The purpose of the dry ice is presumably to lower the pH of the solution by converting potassium carbonate to potassium bicarbonate. 

Buffers are necessary to adjust and maintain the pH. Buffering agents can be salts of a weak acid and a weak base. Examples are ammonium, potassium, sodium carbonates (caustic soda), bicarbonates, and hydrogen phosphates [1345]. Weak acids such as formic acid, fumaric acid, and sulfamic acid also are recommended. Common aqueous buffer ingredients are shown in Table 17-8. 

This process (106— 107) required the incubation of an aqueous mixture of AIR (106), potassium carbonate, and enzyme (AIR carboxylase). The equilibrium of the carboxylation reaction was shown to lie to the left (59JBC1799), but in the presence of 0.3 M aqueous potassium bicarbonate solution, yields of C-AIR (107) approaching 50% were obtained. 

Potassium Bicarbonate. Potassium bicarbonate has become available in commercial quantities for food use. The only reason for using it is that the sodium content of the resulting product is reduced. As the molecular weight of potassium bicarbonate is greater (100.11 for KHC03 compared with 84.01 for NaHC03) some 19% more is required to produce the same volume of carbon dioxide. Potassium bicarbonate is also more expensive. The reaction for its thermal decomposition is ... 

Joosten, G.E.H. and Danckwerts, P.V. Solubility and difussivity of nitrous oxide in equimolar potassium carbonate-potassium bicarbonate solutions at 25 °C and 1 atm, J. Chem. Eng. Data, 17(4) 452-454, 1972. 

Equilibrium perturbation with malic enzyme added to a pH 7.1 solution containing 0.419 mM malate-2-D, 0.079 mM NADPH, 20 mM potassium bicarbonate (3.8 mM carbon dioxide), 20 mM magnesium sulfate, 0.102 mM NADP+, and 3.83 mM pyruvate. NADPH initially disappears within the first 10 min, followed by its reappearance over the ensuing 60 min period. 

The generally accepted mechanisms for the suppression of fires and explosions by alkali metal salts such as potassium chloride, KCl potassium bicarbonate, KHCO3 and potassium carbonate,K2C03 in the form of dry powders or aerosols (smokes) involve heat absorption, endothermic decomposition and radical recombination. 

Potassium bicarbonate is obtained by passing carbon dioxide through a cold, concentrated solution of potassium carbonate ... 

When carbon dioxide is passed into an aqueous solution of potassium carbonate, potassium bicarbonate is produced ... 

Platinum Dichloride Platinum Dioxide Platinum Hexafluoride Platinum Monoxide Platinum Tetrachloride Plutonium Polonium Potassium Potassium Acetate Potassium Bicarbonate Potassium Bisulfide Potassium Borohydride Potassium Bromate Potassium Bromide Potassium Carbonate... 

Mechanism of Action A carbonic anhydrase inhibitor that reduces formation of hydrogen and bicarbonate ions from carbon dioxide and water by inhibiting, in proximal renal tubule, the enzyme carbonic anhydrase, thereby promoting renal excretion of sodium, potassium, bicarbonate, and water. Ocular Reduces rate of aqueous humor formation, lowers intraocular pressure. Therapeutic Effect Produces anticonvulsant activity. 

Nitronium tetrafluoroborate. Acetonitrile, Ammonium carbonate. Potassium carbonate. Diethyl ether, Acetone, Ethyl acetate. Butanol Sulfamic acid, Potassium hydroxide. Ethanol, Nitric acid, Sulfuric acid, Acetone, Isopropyl alcohol Dioxane, Potassium nitrite. Potassium bicarbonate, Tetranitromethane Lead acetate, Sodium azide Sodium azide, Lead acetate. Water... 

Then 100 ml of an ice-cold 10% aqueous potassium bicarbonate solution is added quickly and the aqueous layer is drawn off. The product solution layer is washed with 200 ml of ice water. The carbon tetrachloride solution is dried with anhydrous magnesium sulfate and filtered. The solvent is evaporated under reduced pressure, and the residual dark-colored oil is dissolved in 10 ml of anhydrous ether and cooled to —68°C in a Dry Ice Bath. If a solid forms, it is recrystallized from petroleum ether, which may be warmed to 0°C to effect dissolution followed by cooling to Dry Ice temperatures for precipitation of the purified product. 

Many complexes are unstable in 4.5 N H2SO4, which is used as electrolyte in the fuel cell, even at room temperature. Where tiffs was the case, measurements were carried out in potassium carbonate/potassium bicarbonate buffer solution (pH 9.3). We were thus able to determine the reactivity of a wide range of substances, in particular for the catalytic reduction of oxygen. 

Potassium carbonate is used in the chemical industry as a source of inorganic potassium salts (potassium silicates, potassium bicarbonate), which are used in fertilizers, soaps, adhesives, dehydrating agents, dyes, and pharmaceuticals. Potassium carbonate used to make potassium lye produces soft soaps, which are liquids or semisolids rather than solids. Other uses of potassium carbonate includes use as a fire suppressant in extinguishers, as a C02 absorbent for chemical processes and pollution control, an antioxidant in rubber additives, and in pharmaceutical formulations. 

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