Buxton water

The Bustcn, Bath, and Bristol thermal waters, como under the same category. Annexed is an analysis of the Buxton water just completed by the Editor it differs matarially from the one made by his friend Playfair some time ago, except in the amount of gases — ... 

Macek, K.J., M.A. Lindberg, S. Sauter, K.S. Buxton, and P.A. Costa. 1976. Toxicity of Four Pesticides to Water Fleas and Fathead Minnows. U.S. Environ. Protection Agen. Rep EPA-600/3-76-099. 57 pp. Macko, V., J.A.A. Renwick, and J.F. Rissler. 1978. Acrolein induces differentiation of infection structures in the wheat stem rust fungus. Science 199 442-443. 

Buxton and Harrington [68] used SPE to pre-concentrate explosives and remove matrices. Water samples were passed through commercially available SPE disks. After the extraction step, the SPE disk containing explosives was inserted into... 

Buxton, G.V. Rhodes,T. Sellers, R.M. (1983) Radiation chemistry of colloidal hematite and magnetite in water reductive dissolution by 1-mefhylefhanol radicals (EDTA) iron(ll). J. Chem. Soc. Faraday Trans. 1. 79 2961-2974 Bye, G.C. Howard, C.R. (1971) An examination by nitrogen adsorption of the thermal decomposition of pure and silica doped goefhite. J. Appl. Chem. Biotechnol. 21 324-329... 

Ref Belgranof 1952), 174 Afror Tyne Powder. One of the older Brit "permitted expls NG + NGc 9 AN58, MNN 1, wood meal 9, NaCl 22 water %. It passed the Buxton gallery test and its swing was 2.52, vs 3.27 for Gelignite... 

Errors quoted have been ignored for the sake of clarity, but typically amount to - 25%. Corrections for ionic effect in ethylene glycol—water mixtures have not been made (Buxton and Kemsley). 

Due to its electrophilic properties the OH° reacts at the position with the highest electron density of the target molecule. Detailed information can be found in von Sonntag (1996), which gives a good overview of the degradation mechanism of aromatics by OH° in water. Buxton et al. (1988) showed that the reaction rate constants for hydroxyl radicals and aromatic compounds are close to the diffusion limit. 

The rate constants of the reactions of OH, eaq and H with a large number of compounds have been determined by pulse radiolysis, and their values have been compiled (Buxton et al. 1988). Similarly, a large number of rate constants of the reactions of H02 and 02 are documented (Bielski et al. 1985). A more detailed picture of the radiation chemistry of water is given by Buxton (1987). 

Burkitt MJ, Duncan J (2000) Effects of frans-resveratrol on copper-dependent hydroxyl-radical formation and DNA damage evidence for hydroxyl-radical scavenging and a novel, glutathionesparing mechanism of action. Arch Biochem Biophys 381 253-263 Buxton GV (1987) Radiation chemistry of the liquid state. (1) Water and homogeneous aqueous solutions. In Farhataziz, Rodgers MAJ (eds) Radiation chemistry principles and applications. Verlag Chemie, Weinheim, pp 321-349... 

Swiatla-Wojcik D, Buxton GV (1995) Modeling of radiation spur processes in water at temperatures up to 300°C. J Phys Chem 99 11464-11471... 

Swiatla-Wojcik D, Buxton GV (1998) Modelling of linear energy transfer effects on track core processes in the radiolysis of water up to 300°C. J Chem Soc Faraday Trans 94 2135-2141 Sychev AY, Isak VG (1995) Iron compounds and the mechanisms of the homogeneous catalysis of the activation of O2 and H2O2 and of the oxidation of organic substrates. Russ Chem Rev 12 1105-1129... 

H is the conjugate acid of eaq" [pKa(H") = 9.1 reactions (1), k = 2.2 x 107 dm3 mol-1 s-1 and (2), k = 23 x 1010 dm3 moU1 s 1 (Buxton et al. 1988), for the thermodynamic properties of this system, see Hickel and Sehested (1985)]. Thus, in pure water, the lifetime of eaq is quite long (Hart et al. 1966), even long enough to monitor its presence spectrophotometrically under steady-state 60Co-y-radi-olysis conditions (Gordon and Hart 1964). 

The most difficult aspect of estimating indirect photoreaction rates is finding a measured value of koX or estimating koX for the oxidant and compound of interest. Measured values of koX are usually much preferred to estimated values, but measured values are available only for a small proportion of organic compounds likely to be found in surface waters. Critical compilations of rate constants for oxidant reactions with organic compounds in water appear in Hendry et al. (RO, R02) (1974) Wilkinson et al. (J02) (1995) Buxton et al. (HO and e Aq) (1988) Hendry and Schuetzle (HOz) (1976) Neta et al. (R02) (1990) and Haag and Yao (HO) (1992). 

Rate constants for superoxide ion (02 ) and its conjugate acid HOz as oxidant, reductant, and nucleophile have been measured in several solvents (Hendry and Schuetzle, 1976 Sawyer et al., 1978 Bielski et al., 1985), but few SARs have been developed. Moreover, the reactivity of superoxide ion generally is too low for the oxidant to be important in surface waters. Solvated electrons (e Aq) also form on insolation of DOM (Fischer et. al., 1985 Zepp et. al., 1988), but its concentration is very low, and target compounds are too few to make e (Aq) an important redox agent in surface waters (Buxton et al., 1988). One possible exception is nitroaromatics such as 2,4,6-trinitrotoluene (TNT), which exhibit strong acceleration of photolysis rates in the presence of DOM (Mabey et al., 1983). 

Equations (27) and (28) make it possible to estimate kHO (water) values for many more compounds than are listed (Buxton et al., 1988). 

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