Sodium bicarbonate, NaHCO

Ca(OH)2. calcium hydroxide NaHCOs, sodium bicarbonate Na2CO3 10H2O, sodium carbonate decaliydrate CaS04 2H20, calcium sulfate diliydrate Mg(OH)2. magnesium hydroxide... 

Sodium bicarbonate (NaHCOs). Sodium bicarbonate decomposes between 212 and 284°F giving off CO2 and H2O and forming a sodium carbonate residue. Its gas yield is 267 cm /g. At 287 F or higher, decomposition becomes more rapid, facilitating its use as a blowing agent for such higher-temperature thermoplastics as styrenic polymers. 

Use the molecular volume provided with each compound to calculate its density in g/mL (a) NaHCOs, sodium bicarbonate or sodium hydrogen carbonate (also called baking soda), 0.0389 L/mol (b) I2, iodine, 0.05148 L/mol (c) Hg, liquid mercury, 0.01476 L/mol (d) NaCl, common table salt, 0.02699 L/mol. 

Sodium Bicarbonate. Many soda ash plants convert a portion of their production to sodium bicarbonate [144-55-8], NaHCO. Soda ash is typically dissolved, carbonated, and cooled to crystallize sodium bicarbonate. The mother Hquor is heated and recycled. The soHd bicarbonate is dried in flash or tray driers, screened, and separated into various particle size ranges. Bicarbonate markets include food, pharmaceuticals, catde feed, and fire extinguishers. U.S. demand was approximately 320,000 t in 1989 world demand was estimated at one million metric tons. 

Sodium Bicarbonate. Sodium bicarbonate [144-55-8] NaHCO, is a white crystalline powder. It is odorless, has a saline and shghdy alkaline taste, and is stable in dry air, but slowly decomposes in moist air. Its solubihty is one gram in 10 mL water in hot water it is converted into carbonate, and it is insoluble in alcohol. 

Sodium bicarbonate is a gastric antacid that may cause systemic alkalosis on overdose and may contribute to edema owing to sodium retention. It is useful for systemic acidosis because both deficient ions are present in the same molecule, and it can be used topically as a moist paste or in solution as an antipmritic. Sodium bicarbonate also is an ingredient of many effervescent mixtures, alkaline solutions, etc. One gram of NaHCO neutralizes 115 mL 0.1 NHCl. 

Sodium bicarbonate, NaHCO , is the sodium salt of carbonic acid (II2C03), pfO, = 6.37. Which of the substances shown in Problem 2.43 will react with sodium bicarbonate ... 

Sodium carbonate (Na CO ) is the eleventh most used industrial chemical in the United States. It is commonly used as a bleaching agent and is manufactured in a two-step process. First, ammonia is combined with carbon dioxide to form sodium chloride and water, which reacts to form sodium bicarbonate and ammonium chloride (NH + CO + NaCl + H O —> NaHCOj + NH Cl). Sodium bicarbonate, commonly known as baking soda, is used as a leavening agent in baking, as an antacid to relieve stomach acid, and as a component for fire extinguishers. The second step is known as the Solvay process, wherein the sodium bicarbonate is heated and converted into sodium carbonate (NaHCO A— Na CO + H O + CO ). 

Excretion of drugs will be affected by the pH of the urine. If the urine is acidic, weak bases are ionized and there will be poor re-absorption. With basic urine, weak bases are non-ionized and there is more re-absorption. The pH of the urine can be artificially changed in the range 5-8.5 oral administration of sodium bicarbonate (NaHCOs) increases pH values, whereas ammonium chloride (NH4CI) lowers them. Thus, urinary acidification will accelerate the excretion of weak bases and retard the excretion of weak acids. Making the urine alkaline will facilitate the excretion of weak acids and retard that of weak bases. 

Calcium Salts [Chloride, Sodium Bicarbonate Gluconate] [NaHCOs]... 

As protection against acidic impurities, high-energy mixtures will frequently contain a small percentage of a neutralizer. Sodium bicarbonate (NaHCO 3) and magnesium carbonate (MgCQj) are two frequently-used materials. The carbonate ion, CO3 reacts with H... 

Some consideration was given to appropriate bases for this oxidation system. Pyridine and sodium bicarbonate had been shown to be useful earlier and were included. Additional bases considered were a proton sponge (1,8-Bis(dimethylamino)naphthalene) and, as stated above, pyridine N-oxide. Because of the low solubilities in CXL systems of NaHCOs and the proton-sponge, pyridine was selected for these exploratory studies. 

Alka-Seltzer Sodium bicarbonate NaHCOs H3O+ HCOa + — CO2 + 2H2O... 

Examples of bases, (a) Reactions involving sodium bicarbonate, NaHCO, make baked goods rise, (b) Ashes contain potassium carbonate, K2C03. (c) Soap is made by reacting bases with animal or vegetable oils. The soap itself, then, is slightly alkaline, (d) Powerful bases, such as sodium hydroxide, NaOH, are used in drain cleaners. 

Sodium Bicarbonate (NaHCO.) 100-140 135 Endo LDPE. EVA, FPVC. TPE... 

An older nomenclature system, still in use to some extent, uses the word acid to denote an acid salt. Also, the prefix bi- may be used for an acid salt of an acid with two ionizable hydrogen atoms. Thus, NaHCOs can be called sodium bicarbonate or sodium acid carbonate instead of sodium hydrogen carbonate (Figure 6.5). 

C,H,-C0 0.N C(NH,HN,0)-aNH,) N-0-OC-CsH, mw 370.32, N 22.70% yel ndls (from glacial acetic acid) mp — explodes at 155°. This. compd was obtd, in addn to col ndls of benzoylguanidine benzoate [QH,. C0-NH-C(NHj) N-0 0C-C.H5 ], when dihydroxyguanidine and benzoyl chloride reacted in the presence of sodium bicarbonate. Attempts to methylate or benzoylate azodi-carboxylamide dioxime by means of methyl sulfate or benzoyl chloride either in NajCO, or NaHCOs soln were without success. The yel material isolated was purified by repeated shaking with acet until it was sol in dil NaOH, which quickly caused decompn into benzoic acid, nitrogen, and hydroxy-carbamide. The col purified crysts of the benzoylguanidine benzoate decompd at 162-3°... 

Sodium bicarbonate, a weak base, is used because a strong base like sodium hydroxide can damage the resin.) A fO.O wt% aqueous NaHCOs solution at 21°C pumped from the NaHCOs feed drum (Step II) is augmented by a clean water stream at 60°C, and the combined stream is fed to the tank. Enough bicarbonate solution is fed to neutralize all the HCI in the wetcake, and enough additional water is added to make a 15.0 wt% CPVC slurry in the vessel. 

Step 11. The sodium bicarbonate solution fed to the resin neutralizer (Step 10) is produced by dissolving NaHCO powder from 25-kg bags in clean water in the NaHCOa makeup tank, an agitated batch vessel. This makeup tank is not jacketed like the NaOH makeup tank, as the heat of solution of sodium bicarbonate is low enough for the heat generated in the tank to be neglected. Batches of solution are pumped from the makeup tank to the NaHCOj feed drum, and solution is pumped continuously from the feed drum to the resin neutralizer. 

NaHCOs under phase-transfer conditions,or with sodium bicarbonate with ultrasound. 

Weak acids and bases will also undergo neutralization reactions. The reaction of the acetic acid (HAc) in vinegar with the sodium bicarbonate (NaHCOs) in baking soda produces water, sodium ions (Na+), acetate ions (Ac), and carbon dioxide gas (CO2). The reaction between baking soda and acids in dough creates bubbles of carbon dioxide that make cakes and cookies rise and become fluffy. 

Soluble, effervescent tablets are prepared by compression. In addition to active ingredients, they contain mixtures of acids (citric acid, tartaric acid) and sodium bicarbonate (NaHCOs) that release carbon dioxide when dissolved in water. The United States Pharmacopeia (USP) 24 includes the following seven monographs Acetaminophen for Effervescent Oral Solution Aspirin Effervescent Tablets for Oral Solution Potassium Bicarbonate Effervescent Tablets for Oral Solution Potassium Bicarbonate and Potassium Chloride for Effervescent Oral Solution Potassium Bicarbonate and Potassium Chloride Effervescent Tablets for Oral Solution Potassium and Sodium Bicarbonates and Citric Acid for Oral Solution and Potassium Chloride, Potassium Bicarbonate, and Potassium Citrate Effervescent Tablets for Oral Solution. ... 

Sodium bicarbonate Sodium bicarbonate (NaHCOs) is an odorless, white crystalline powder with a saline, slightly alkaline taste. A variety of particle-size grades of powders and granules are available. The carbon dioxide yield is approximately 52% by weight. At RH below approximately 80% (at room temperature), the moisture content is less than 1%. Above 85% RH, it rapidly absorbs an excessive amount of water and may start to decompose. Its solubility in water is 1 part in 11 parts at 20°C, and it is practically insoluble in 95% ethanol at 20°C. When heated to 250-300°C, NaHCOs decomposes and is converted into anhydrous sodium carbonate. However, thisprocess is both time-and temperature-dependent, commencing at about 50°C. The reaction proceeds via surface-controlled kinetics, and when NaHCOs crystals are heated for a short period of time, very fine needle-shaped crystals of anhydrous sodium carbonate appear on the surface. ... 

We attempted the palladium-catalyzed ring closure of 27a (Table 5). Treatment of 27a with palladium(Tf) acetate [Pd(OAc)2] (30 mol%) in the presence of triethylphosphite [( tO)3P] and sodium bicarbonate (NaHCOs) in aqueous tetrahydrofuran (THF) afforded the desired cyclized product 28a albeit in a poor yield (30%) (Table 5, Entry 1). Both the lack of base or the use of a strong base (NaH) in place of NaHCOs were detrimental, yielding thiophene 44 or 2-oxazolidinone derivative 45, respectively (Table 5, Entries 2 and 3). 

NaHCOs is also known as sodium bicarbonate, bicarbonate of soda, or baking soda. 

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