Monochloroacetate ions

CH2ClCOO (aq.). The value for aqueous monochloroacetate ion is obtained from that for the aqueous sodium salt. 

Figure 16), better known as ferric wheel [11,48,53]. The wheel is prepared in methanol solution from the reaction between [Fe30(02CCFl2Cl)6(H20)3](N03) and Fe(N03)3-9H20. Four p2-OMe donors and two monochloroacetate ions link three Fe(lII) ions each out of the 10 Fe(Ill) ions of 25 and is unoccupied in the center. 

For many years fluorine has been deterrnined by the Willard-Winters method in which finely ground ore, after removal of organic matter, is distilled with 72% perchloric acid in glass apparatus. The distillate, a dilute solution of fluorosiUcic acid, is made alkaline to release fluoride ion, adjusted with monochloroacetic acid at pH 3.4, and titrated with thorium nitrate, using sodium a1i2arine sulfonate as indicator. 

DeMent (Ref) proposed to use the following Co ion contg mixts as smoke-producing pyrotechnic compns a)Co stearate 2.0, K chlorate 10.0 to 12.0 Amm acid fluoride 4.0 to 8.0 parts. This compn, when ignited by a flame, produced a heavy, voluminous fine white smoke b)When using monochloroacetic acid in previous mixt, instead of fluoride, the color of smoke produced was blue-white c)Equal parts of Co chloride, K bromate, K bromide, sulfur, K chlorate K acid sulfate burned with the emission of a green to green-brown smoke d)Equal parts of Co nitrate, K bromate, K bromide, sulfur, K chlorate K acid sulfate burned with the emission of grn to gm-bm smoke e)A mixt of Co chloride 1.0, K chlorate 2.0,K iodate 1.0, K iodide 1.0 sulfur 1.5 parts burned with evolution of a heavy voluminous deep violet smoke Ref J.DeMent, USP 2995526 (1961), p8... 

Instead of monochloroacetic acid, the condensation with a primary amine can be done using methyl bromoacetate. This procedure was used for the syntheses of /J-methoxyethyliminodiacetic acid /J-methoxyethylamine, methyl bromoacetate and potassium carbonate were reacted without solvent with formation of the corresponding ester (equation 6). This was separated, purified by distillation and hydrolyzed with a Ba(OH)2 solution. The separation of the acid from die solution was made after quantitative removal of barium ions with sulfuric acid.10... 

B) Ionization Constants. Determine the pH of 0.1 solutions of acetic, chloroacetic, and trichloroacetic acids. Convert the pH to hydrogen-ion concentration as moles per liter then calculate the ionization constants for acetic and monochloroacetic acid. 

Figure 14.8 Proton transfer mechanism ofthe loose complexes R0H---(H20) ---B with a sequential, von Grotthuss-type, hopping of protons through water bridges. For H PTS and monochloroacetate the first transfer to the water bridge forming the hydronium ion HjO+ is ultrafast, and the second transferto the base is slower. (Adapted from Ref [136].)...

Figure 4.17. Separation of a mixture of inorganic and organic anions by gradient elution ion chromatography with conductivity detection using a micromembrane suppressor. A variable rate gradient from 0.5 mM to about 40 mM sodium hydroxide on an lonPac ASH column was used for the separation. Peak identification 1 = isopropylmethylphosphonate 2 = quinate 3 = fluoride 4 = acetate 5 = propionate 6 = formate 7 = methylsulfonate 8 = pyruvate 9 = chlorite 10 = valerate 11 - monochloroacetate 12 - bromate 13 = chloride 14 = nitrite 15 = trifluoroacetate 16 = bromide 17 = nitrate 18 = chlorate 19 = selenite 20 = carbonate 21 = malonate 22 = maleate 23 = sulfate 24 = oxalate 25 = ketomalonate 26 = tungstate 27 = phthalate 28 = phosphate 29 = chromate 30 = citrate 31 = tricarballylate 32 = isocitrate 33 = cis-aconitate and 34 = trans-aconitate. Each ion is at a concentration between 1 to 10 mg/1. (From ref. [417]. Marcel Dekker).

Investigation into the formation of carboxymethyl ethers of polysaccharides has continued, on account of the great utility of these derivatives as ion-exchange materials and polyelectrolytes. As expected, a whole series of polysaccharide derivatives of different degrees of substitution can be prepared by variation of the reaction conditions and molar proportions of monochloroacetic acid. " Published reports include the preparation of various carboxymethyl ethers of starches, amyloses, lichenan, pachymans, and chitin and introduction of the carboxymethyl group into polysaccharide derivatives constitutes a useful way of raising their solubility in water. By combining the introduction of alkyl and carboxy-... 

Several reports concern the formation of organic ligand complexes of iron(iii). The variation of rate with ligand concentration in the reaction with mandelic acid > is interpreted as a pre-equilibrium ion-pair formation followed by dissociative complex formation within the ion-pair, rather than as simple 5 n2 formation. This interpretation is similar to that proffered for formation of malonate and oxalate complexes of chromium(iii) (see above). Rates of reaction of iron(iii) with a variety of phenols are all very similar, suggesting that iron(iii)-water bond breaking is rate determining here also. Sulphosalicylate reacts with FeOH + by the same rate-determining loss of water from the iron(m). Rates of formation of iron(iii) complexes with acetate, monochloroacetate, and propionate have been reported. ... 

Using an ion-exchange separation in conjunction with a suppressed electrical conductivity detector, based on an injected volume of 100 pi and a 3 1 signal-to-noise ratio, it is possible to detect haloacetic acids down to the following limits monochloroacetic acid = 8.0 ppb, dichloroacetic acid = 16.0 ppb, trichloroacetic acid = 80.0 ppb, trifluoroacetic acid = 12.0 ppb, bromoacetic acid = 21.0 ppb, and dibromo-acetic acid = 30.0 ppb. 

Better results were obtained with catalysts of the type of quaternary phosphonium nickel halogenides or the corresponding ammonia compounds [408, 409]. Nickel bromide and nickel iodide are only soluble in butyl acrylate/butanol mixtures in amounts which are insufficient for the maintenance of the catalytic process. As mentioned in patents [408, 409], tertiary and quaternary complex compounds supply the required concentration of nickel and halogen ions for a continuous reaction. Many of the carbonylations, especially the stoichiometric reactions with Ni(CO)4 are carried out in the presence of water and acids. Jones [369] investigated the efficiency of the monobasic acids and showed hydrochloric acid and acetic acid to be of the same efficiency, whereas trichloro acetic acid is inefficient. He concludes that not the protons of the acids but the anions are of importance in the reaction mechanism. Apart from hydrochloric acid and acetic acid [345], sulfuric acid, aqueous phosphoric add, formic acid [367] and monochloroacetic acid are suited. A number of other organic acids [367] are ineffective. Acetic acid may be used in less than the equivalent amount because the unsaturated acid formed in the hydrocarbox-ylation [367] may replace acetic acid. 

Stationary phase Silica gel G. Mobile phase M, M2, Afj, and M4 are 0.1 M solutions of trichloroacetic, dichloroacetic, monochloroacetic and acetic acids respectively. Detection Standard spot test reagents. Remarks The effects of concentration, pH and chlorosubstitueni groups of the mobile phase on the Rf values of metal ions were examined. 

The propionate ion forms somewhat stronger complexes than the acetate ion with Th, and H", while the opposite is true for monochloroacetate... 

---