Alberty

Procedure. A study on the partial molal volume of ZnCl2 solutions gave the following data (Alberty, 1987)... 

Diphenyl disulfide (phenyl disulfide) [882-33-7] M 218.3, m 60.5 . Crystd from MeOH. [Alberti et al. J Am Chem Soc 108 3024 1986]. Crystd repeatedly from hot diethyl ether, then vac dried at 30° over P2O5, fused under nitrogen and re-dried, the whole procedure being repeated, with a final drying under vac for 24h. Also recrystd from hexane/EtOH soln. [Burkey and Griller 7 Am Chem Soc 107 246 1985.]... 

It has been recrystd from H2O (fine needles) and is freely soluble in boiling H2O. Crysts also from H2O by addition of acetone. Purified by chromatography on Dowex 1 (in formate form), eluting with 0.25M formic acid. It was then adsorbed onto charcoal (which had been boiled for 15min with M HCI, washed free of chloride and dried at 100°), and recovered by stirring three times with isoamyl alcohol/H20 (1 9 v/v). The aqueous layer from the combined extracts was evaporated to dryness under reduced pressure, and the product was crystallised twice from hot H2O. [Morrison and Doherty Biochem J19 433 7967]. It has A-max 259nm (e 15,400) in H2O at pH 7.0. [Alberty et al. J Biol Chem 193 425 7957 Martell and Schwarzenbach Heh Chim Acta 39 653 7956]. The acridinium salt has m 208° [Baddiley and Todd J Chem Soc 648 1947 Pettit Synthetic Nucleotides, van Nostrand-Reinhold, NY, Vol 1 252 1972 NMR Sarma et al. J Am Chem Soc 96 7337 1974 Norton et al. J Am Chem Soc 98 1007 1976 IR of diNa salt Miles Biochem Biophys Acta 27 324 1958],... 

Pyridoxal hydrochloride [65-22-5] M 203.6, m 176-180 (dec), pK 4.23 (3-OH), pK (Pyridinium+), pK 13.04 (CHjOH ). Dissolve in water and adjust the pH to 6 with NaOH. Set aside overnight to crystallise. The crystals are washed with cold water, dried in a vacuum desiccator over P2O5 and stored in a brown bottle at room temperature. [Fleck and Alberty J Phys Chem 66 1678 7962.]... 

Alberty, R. A., 1968. Effect of pH and metal ion concentration on die equilibrium hydroly.si.s of adeno.sine tripho.sphate to adeno.sine dipho.sphate. 

Alberty, R. A., 1969. Standard Gibb.s free energy, enthalpy, and entropy change.s a.s a function of pH and pMg for reaction.s involving adeno.sine pho.sphate.s. of Biological Chemistry 244 3290-3302. 

Daniels, F., and Alberty, R. A., Physical Chemistry, Fourth Editon,John Wiley and Sons, New York, 1975. 

R.A. Alberty, R.J. Silbey, Physical Chemistry, John Wiley, New York, 1996. 

There are two principal chemical concepts we will cover that are important for studying the natural environment. The first is thermodynamics, which describes whether a system is at equilibrium or if it can spontaneously change by undergoing chemical reaction. We review the main first principles and extend the discussion to electrochemistry. The second main concept is how fast chemical reactions take place if they start. This study of the rate of chemical change is called chemical kinetics. We examine selected natural systems in which the rate of change helps determine the state of the system. Finally, we briefly go over some natural examples where both thermodynamic and kinetic factors are important. This brief chapter cannot provide the depth of treatment found in a textbook fully devoted to these physical chemical subjects. Those who wish a more detailed discussion of these concepts might turn to one of the following texts Atkins (1994), Levine (1995), Alberty and Silbey (1997). 

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