Carbonate acidizing formic acid

More complicated catemer patterns are frequently encountered in organic crystals. Particularly interesting examples are the first two carbonic acids, formic acid and acetic acid. Both, as with most other carbonic acids, form doubly hydrogen-bonded, cyclic dimers in the vapor phase, but chains with one hydrogen bond linking the monomers in the molecular crystal [34-40]. The structures are sketched in Figure 8.11. Propionic acid [316] and others... 

Common names for some aldehydes are widely used. The common names for the aldehydes are derived from the common names of the carboxylic acids (see Table 19.7). The -ic acid or -oic acid ending of the acid name is dropped and is replaced with the suffix -aldehyde. Thus the name of the one-carbon acid, formic acid, becomes formaldehyde for the one-carbon aldehyde ... 

Most weak base anion exchangers adsorbweak organic acids such as formic acid [64-18-6] and acetic acid [64-19-7] but do not remove weak organic acids such as carbonic acid [463-79-6] or siHcic acid [7669-41 ]. 

In eadier Hterature carbonochloridic esters are referred to as chloroformates or chlorocarbonates because of the stmctural parallel with formic acid [64-18-6]., chloroformic acid, and carbonic acid. Before 1972, chloroformates were indexed in Chemicaly4bstracts, Eighth Collective Index, under formic acid, chloroesters whereas, in the Ninth Collective Index (Dec. 1990), they are referred to as carbonochloridic acid esters. Table 1 fists the common names of carbonochloridates or chloroformates, the CAS Registry Numbers, and the formulas. 

Because the solution is capable of absorbing one mole of carbon monoxide per mole of cuprous ion, it is desirable to maximize the copper content of the solution. The ammonia not only complexes with the cuprous ion to permit absorption but also increases the copper solubiUty and thereby permits an even greater carbon monoxide absorption capacity. The ammonia concentration is set by a balance between ammonia vapor pressure and solution acidity. Weak organic acids, eg, formic, acetic, and carbonic acid, are used because they are relatively noncorrosive and inexpensive. A typical formic acid... 

H2CO3 (carbonic acid) aqueous phase HC2H3O2 (acetic acid) aqueous, gas phases HCHOz (formic acid) aqueous, gas phases H2C2O4 (oxalic acid) aerosol particles solid phase RCCX3H (many carboxylic acids)... 

In this chapter, we have summarized (recent) progress in the mechanistic understanding of the oxidation of carbon monoxide, formic acid, methanol, and ethanol on transition metal (primarily Pt) electrodes. We have emphasized the surface science approach employing well-defined electrode surfaces, i.e., single crystals, in combination with surface-sensitive techniques (FTIR and online OEMS), kinetic modeling and first-principles DFT calculations. 

Mixed acid systems are blends of mineral acids and organic acids. Combinations that have been used in carbonate acidizing include acetic acid/HCl and formic acid/HCl. While these are less corrosive than hydrochloric acid alone, the organic acid may not react completely with the rock. Blends of formic acid and hydrofluoric acid have been used in high temperature sandstone acidizing and are less corrosive than HC1/HF blends. 

Addition of bases or acids to nitromethane renders it susceptible to initiation by a detonator. These include aniline, diaminoethane, iminobispropylamine, morpholine, methylamine, ammonium hydroxide, potassium hydroxide, sodium carbonate, and formic, nitric, sulfuric or phosphoric acids. 

The synthesis of cellulose by A. xylinum from various polyalcohols14 is accompanied by the formation of carbon dioxide, formic acid, nonvolatile acids, ketoses and sometimes ethanol. The much greater variety of substrates suitable for cellulose synthesis, as compared with the small number for dextran or levan, may account for the widespread natural occurrence of cellulose. 

Photolytic. Carbon monoxide, formic and hydrochloric acids were reported to be photooxidation... 

Chemical/Physical. At temperatures greater than 189.5 °C, decomposes to carbon dioxide, carbon monoxide, formic acid, and water (Windholz et al, 1983). Ozonolysis of oxalic acid in distilled water at 25 °C under acidic conditions (pH 6.3) yielded carbon dioxide (Kuo et al., 1977). 

Some commonly used buffers, such as sodium and potassium phosphate, are incompatible with ELSD, but there are ready alternatives. For example, ammonium acetate has similar buffering properties to potassium phosphate, and ammonium carbonate, ammonium formate, pyridinium acetate, and pyridinium formate are options for different pH ranges. Typical mobile phase modifiers that do not meet the volatility criteria can be replaced by a wide variety of more volatile alternates. For example, phosphoric acid, commonly used as an acid modifier fo control pH and ionization, can be replaced by trifluoroacetic acid other acids that are sufficiently volatile for use with FLSD include, acetic, carbonic, and formic acids. Triethylamine, commonly used as a base modifier, is compatible with FLSD other base modifiers that can be used are ethylamine, methylamine, and ammonium hydroxide [78]. 

The C,-synthon is usually a carboxylic acid or a derivative of a carboxylic or carbonic acid and introduces substituent R . An example is the reaction of 4-oxo-6-methyl-HP (16) and formic acid in Scheme 9 (59JOC787). 

The precision of the ICE method was determined by analyzing six replicates of two standard solutions containing strong acids (i.e., H2S0i ) and several weak acids (i.e., formic acid, acetic acid and carbonic acid). Carbonic acid is present as a result of the use of Na2C03 n the standard solution matrix (as in the collection medium) and dissolution of atmospheric carbon dioxide (Figure 4). At formic acid concentrations of 5.0 and 10 mg/L, the measured mean concentrations (Table III) were 5.08 and... 

The detection limit for a 100 yL sample injection volume at 30 ymhos full scale sensitivity is estimated at 0.5 yg/mL. Concentration of samples by freeze-drying affords better detection limits with minimal loss of formic acid. Acetic and carbonic acids are also analyzable under these conditions. 

Just as by the reducing action of hydrogen on carbon dioxide formic acid, formaldehyde, methyl alcohol and methane may be directly or... 

Some synthetic pathways require the addition of single carbon groups. These "one-carbon units can exist in a variety of oxidation states. These include methane, methanol, formaldehyde, formic acid, and carbonic acid. It is possible to incorporate carbon units at each of these... 

Isbell and co-workers (51) have tried to minimize the oxygen reaction and to maximize the peroxide reaction. When a large excess of peroxide and a low temperature were maintained, they found that the monosaccharides are converted almost quantitatively to formic and two-carbon acids. Table II presents results for the peroxide oxidation of 14 sugars. The total acid produced from aldo-hexoses under favorable conditions is about six moles, consisting almost entirely of formic acid. Aldopentoses react more rapidly than aldo-hexoses and yield about five moles of formic acid per mole of pentose. Fructose and sorbose yield approximately five moles of total acid of which four moles are formic acid. Glycolic acid was identified qualitatively but not determined quantitatively. L-Rham-nose and L-fucose yield about five moles of acid, including four moles of formic acid. Acetic acid was identified only qualitatively. 

The acidity of wine is due to organic acids, some of which are fixed— tartaric, malic, succinic—whilst others, such as acetic and also formic, butyric and propionic, which are found in minimal proportions, are volatile carbonic acid plays no part in the acidity of wine. 

At higher temperatures, carbon dioxide, formic acid, oxalic acid, glycolic acid, hydroxymalonic acid, glyceric acid, and other acids were shown to be formed. The formation of carbon dioxide is ascribed to decarboxylation of 38 oxalic acid and D-erythronic acid arise from cleavage of the C-2-C-3 bond compound 39 is cleaved to glyoxylic acid plus D-erythronic acid. Compound 40 is oxidized further to D-g7ycero-2,3-pentodiulosonic acid and is subsequently cleaved to oxalic and glyceric acids. 

At ambient temperatures CO is only slightly soluble in water. This behavior is in contrast to the case for carbon dioxide, which dissolves and is easily hydrated to carbonic acid and its conjugate bases. The simple solution of CO in water in accord with its Henry s law constant continues to about 250°C. At that temperature the rate of hydration becomes significant, and formic acid is formed. However the acid is thermally unstable, and subsequently decomposes to C02 and H2. 

When a nucleophile containing a heteroatom reacts at a carboxyl carbon SN, reactions occur that convert carboxylic acid derivatives into other carboxylic acid derivatives, or they convert carbonic acid derivatives into other carbonic acid derivatives. When an organometallic compound is used as the nucleophile, SN reactions at the carboxyl carbon make it possible to synthesize aldehydes (from derivatives of formic acid), ketones (from derivatives of higher carboxylic acids), or—starting from carbonic acid derivatives—carboxylic acid derivatives. Similarly, when using a hydride transfer agent as the nucleophile, SN reactions at a carboxyl carbon allow the conversion of carboxylic acid derivatives into aldehydes. 

Calvert and Hanst88 using infrared analysis, have also re-investigated the photooxidation of acetaldehyde at 20°C. using 3130 A. radiation. Acetaldehyde pressures were chiefly about 42.5 nun., but the oxygen pressure was varied from 0 to 745 mm. Analyses were made for carbon monoxide, carbon dioxide, formic acid, methanol, acetic acid, peracetic acid, acetyl peroxide, methyl hydroperoxide, and unreacted acetaldehyde (Table X). Chains were short. Although they do not detect methyl hydroperoxide or diacetyl peroxide, the non-observance of a peroxide does not necessarily mean it is not formed. The decomposition of hydroperoxides on the smallest particle of catalyst is remarkably fast. 

While these experiments, which were carried out without giving a theoretical insight into the nature of the electrochemical reaction, yielded almost all the possible oxidation products in the oxidation of methyl alcohol, Elbs and Brunner 2 have discovered a method which gives 80% of the current yield in formaldehyde. This is exactly the substance which could not be proven present up to that time among the electrolytic oxidation products of methyl alcohol. Elbs and Brunner electrolyzed an aqueous solution of 160 g. methyl alcohol and 49 to 98 g. sulphuric acid in a litre. They employed a bright platinum anode in an earthenware cylinder, using a current density of 3.75 amp.1 and a temperature of 30°. Only traces of formic acid and carbonic acid and a little carbon monoxide, aside from the 80 per cent, of formaldehyde, were formed. Plating the platinum anode with platinum decreased the yield of formaldehyde at the expense of the carbon dioxide. With an anode of lead peroxide the carbon dioxide exceeded the aldehyde. 

Acetone, acetic acid, formic acid, and carbonic acid are formed. The oxidation takes place more easily than in the case of the primary alcohols, and yields up to 70% acetone, which, however, is readily oxidized further. In alkaline electrolytes the alcohols are converted at the anode into complicated condensation products of the aldehydes. 

Acetone.—Friedel,4 by electrolyzing a sulphuric-acid solution of acetone, obtained carbonic acid, acetic acid, and formic acid. Mulder 5 and Riche 6 were able to isolate mono- and dichloracetone from the hydrochloric-acid electrolyte, and monobrom,acetone from a hydrobromic-acid solution. 

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