Titlebook: Buffers for pH and Metal Ion Control; D. D. Perrin,Boyd Dempsey Book 1974 D. D. Perrin and Boyd Dempsey 1974 Ampholyte.Chromat.Titration.a

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The Theory of Buffer Action,An acid is a species such as the ammonium ion or the acetic acid molecule which has a tendency to lose a proton. A base (such as the ammonia molecule or the acetate anion) is able to accept a proton. Hence for every acid, HA, there is a conjugate base, A., and for every base, B, there is a conjugate acid, BH..

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Appendices,Tables 10.1 and 10.2 enable buffer tables to be constructed for use at a constant ionic strength of 0.1 for monoacidic bases or monobasic acids, given the appropriate ‘practical’ p.’. Where necessary, this can be calculated from the thermodynamic value in Appendix III by using Table 2.3.

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Applications of pH Buffers, is clearly the most important single factor in choosing a buffer for any particular application and reference to lists of p. values such as those given in Appendix III provides a rapid indication of possible buffer substances.

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Practical Limitations in the use of Buffers,se. For a buffer to be effective, its pH must be within the range p. ± 1, or preferably, within p. ± 0.5. The former scarcity of buffer substances with a pH range 6 to 8 frequently led to the use of buffers such as phosphate or Tris in pH regions where they had little buffer capacity.

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Metal-Ion Buffers,0.M are difficult to maintain in the presence of adventitious complexing agents, hydrolytic equilibria, adsorption and, possibly, contamination. Many problems can be overcome by the use of metal-ion buffers which provide a controlled source of free metal ions in a manner similar to the regulation of hydrogen ion concentration by pH buffers.

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https://doi.org/10.1007/978-94-009-5874-6Ampholyte; Chromat; Titration; amines; biochemistry; chemical reaction; chromatography; electrolyte; electro

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