Bicarbonate ion

A further peculiarity of the Group I and II carbonates is the ability to form the hydrogencarbonate or bicarbonate ion HCOj ... 

Carbonic acid is formed when carbon dioxide reacts with water Hydration of car bon dioxide is far from complete however Almost all the carbon dioxide that is dis solved m water exists as carbon dioxide only 0 3% of it is converted to carbonic acid Carbonic acid is a weak acid and ionizes to a small extent to bicarbonate ion... 

A second molecule of acetyl coenzyme A reacts with carbon dioxide (actually bicarbonate ion at biological pH) to give malonyl coenzyme A... 

Amphiprotic Species Some species can behave as either an acid or a base. For example, the following two reactions show the chemical reactivity of the bicarbonate ion, HC03, in water. 

Equation 2 shows that the acid dissociates to form bicarbonate ions and hydrogen ions ... 

The alkalinity is determined by titration of the sample with a standard acid (sulfuric or hydrochloric) to a definite pH. If the initial sample pH is >8.3, the titration curve has two inflection points reflecting the conversion of carbonate ion to bicarbonate ion and finally to carbonic acid (H2CO2). A sample with an initial pH <8.3 only exhibits one inflection point corresponding to conversion of bicarbonate to carbonic acid. Since most natural-water alkalinity is governed by the carbonate—bicarbonate ion equiUbria, the alkalinity titration is often used to estimate their concentrations. 

Obtaining maximum performance from a seawater distillation unit requires minimising the detrimental effects of scale formation. The term scale describes deposits of calcium carbonate, magnesium hydroxide, or calcium sulfate that can form ia the brine heater and the heat-recovery condensers. The carbonates and the hydroxide are conventionally called alkaline scales, and the sulfate, nonalkaline scale. The presence of bicarbonate, carbonate, and hydroxide ions, the total concentration of which is referred to as the alkalinity of the seawater, leads to the alkaline scale formation. In seawater, the bicarbonate ions decompose to carbonate and hydroxide ions, giving most of the alkalinity. 

The kinetics of the formation of the magnesium hydroxide and calcium carbonate are functions of the concentration of the bicarbonate ions, the temperature, and the rate of release of CO2 from the solution. At temperatures up to 82°C, CaCO predominates, but as the temperature exceeds 93°C, Mg(OH)2 becomes the principal scale. Thus, ia seawater, there is a coasiderable teadeacy for surfaces to scale with an iacrease ia temperature. 

In another option, the hydrogen ion from added acid decomposes the bicarbonate ions. 

The component reactions in eqn. (2) are very fast, and the system exists in equilibrium. Additional carbon dioxide entering the sea is thus quickly converted into anions, distributing carbon atoms between the dissolved gas phase, carbonate and bicarbonate ions. This storage capacity is clear when the apparent equilibrium constants for the two reactions in eqn. (2) are examined, namely... 

Potassium cyanate [590-28-3] M 81.1, d 2.05, pK 3.46 (for HCNO). Common impurities include ammonia and bicarbonate ion (from hydrolysis). Purified by preparing a saturated aqueous solution at... 

The systematic name for bicarbonate ion is hydrogen carbonate. Thus, the systematic name for sodium bicarbonate (NaHC03) is sodium hydrogen carbonate. 

FIGURE 1.19 Carbonic anhydrase, a representative enzyme, and the reaction that it catalyzes. Dissolved carbon dioxide is slowly hydrated by water to form bicarbonate ion and... 

The enzyme carbonic anhydrase promotes the hydration of COg. Many of the protons formed upon ionization of carbonic acid are picked up by Hb as Og dissociates. The bicarbonate ions are transported with the blood back to the lungs. When Hb becomes oxygenated again in the lungs, H is released and reacts with HCO3 to re-form HgCOj, from which COg is liberated. The COg is then exhaled as a gas. 

Fig. 4. The pH-rate profile for the hydration of 2-hydroxypteridine at 20°. Deviations at low rates are due to catalysis by boric acid and bicarbonate ion present in the buffers.

Among one of the more unusual side effects noticed as the use of the sulfonamides became widespread was the increased urine output of many patients treated with these drugs. The fact that the urine was unusually alkaline led to the suspicion, later (Confirmed by independent means, that these agents were responsible for partial inhibition of the enzyme carbonic anhydrase. Inhibition of this enzyme causes increased excretion of sodium and bicarbonate ions as well as water, in effect bringing about diure-... 

As the pH is further reduced to 4.3, the acid then reacts with the bicarbonate ions to form carbon dioxide and water. 

A 0-9% salt solution is considered to be isotonic with blood. Other electrolytes present include bicarbonate ions (HCOj ) and small amounts of potassium, calcium, magnesium, phosphate, sulphate and organic acid ions. Included among the complex compounds and present in smaller amounts are phospholipids, cholesterols, natural fats, proteins, glucose and amino acids. Under normal conditions the extracellular body fluid is slightly alkaline with a pH of 7-4. ... 

Those waters in which the carbon dioxide content is in excess of that required as bicarbonate ion to balance the bases present are among the most aggressive of the fresh waters. Hard waters usually, though not invariably, deposit a carbonate scale and are generally not appreciably corrosive to cast iron, corrosion rates of less than 0-02 mm/y being frequently encountered. Water-softening processes do not increase the corrosivity of the water provided that the process does not result in the development of an excess of dissolved carbon dioxide. 

As indicated above, the bicarbonate ion inhibits the process, which does not occur, therefore, in many supply waters attack is most likely in waters which by nature or as a result of treatment have a low bicarbonate content and relatively high chloride, sulphate or nitrate content. The number of points of attack increases with the concentration of aggressive anions and ultimately slow general corrosion may occur. During exposure of 99-75% tin to sea-water for 4 years, a corrosion rate of 0-0023 mm/y was observed . Corrosion in soil usually produces slow general corrosion with the production of crusts of oxides and basic salts this has no industrial importance but is occasionally of interest in archaeological work. 

Step 1 of Figure 29.13 Carboxylation Gluconeogenesis begins with the carboxyl-afion of pyruvate to yield oxaloacetate. The reaction is catalyzed by pyruvate carboxylase and requires ATP, bicarbonate ion, and the coenzyme biotin, which acts as a carrier to transport CO2 to the enzyme active site. The mechanism is analogous to that of step 3 in fatty-acid biosynthesis (Figure 29.6), in which acetyl CoA is carboxylated to yield malonyl CoA. 

Reaction (25) also provides a basis for understanding the removal of acid properties. If COf2 readily forms bicarbonate ion,t HCO3, then reaction (26) is likely ... 

We see that the existence of the stable bicarbonate ion, HCO foqj produces the chemical species, OH (aq) in common with solutions of the hydroxides. We can postulate that OH (ag) accounts for the slippery feel and bitter taste of the basic solutions. The stability of bicarbonate ion also explains the removal of acid properties through reaction (26). 

The combination of reaction (18) and (16) shows how carbon dioxide enhances the solubility of calcium carbonate by removing carbonate ion to form bicarbonate ion,... 

Beryllium difiuoride, dipole in, 293 Berzelius, Jons, 30 Bessemer converter, 404 Beta decay, 417 Bela particle, 417 Bicarbonate ion, 184 Bidentaie. 395 Billiard ball analogy, 6, 18 and kinetic energy, 114 Billiard ball collision, conservation of energy in, 114 Binding energy, 121, 418 Biochemistry, 421 Bismuth, oxidation numbers, 414 Blast furnace, 404 Bohr, Niels, 259 Boiling point, 67 elevation, 325 normal, 68... 

Reaction of COJ with H20 may yield formate and/or bicarbonate ions. 

In experiments where Mono Lake water was acidified to remove carbonate and bicarbonate ions and again adjusted to pH 10, more than 90 percent of the soluble plutonium moved to the sediment phase. When carbonate ion concentration was restored, the plutonium returned to solution—strong evidence of the importance of inorganic carbon to solubility in that system(13). Early studies with Lake Michigan water, which has low DOC, had also implicated bicarbonate and carbonate as stabilizing ligands for plutonium at pH 8(14). This latter research characterized the soluble species as mainly anionic in character. 

The complexation of Pu(IV) with carbonate ions is investigated by solubility measurements of 238Pu02 in neutral to alkaline solutions containing sodium carbonate and bicarbonate. The total concentration of carbonate ions and pH are varied at the constant ionic strength (I = 1.0), in which the initial pH values are adjusted by altering the ratio of carbonate to bicarbonate ions. The oxidation state of dissolved species in equilibrium solutions are determined by absorption spectrophotometry and differential pulse polarography. The most stable oxidation state of Pu in carbonate solutions is found to be Pu(IV), which is present as hydroxocarbonate or carbonate species. The formation constants of these complexes are calculated on the basis of solubility data which are determined to be a function of two variable parameters the carbonate concentration and pH. The hydrolysis reactions of Pu(IV) in the present experimental system assessed by using the literature data are taken into account for calculation of the carbonate complexation. 

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