Analytical ChemistryWiley, 14 mar 2003 - 848 pagine Extensively revised and updated with a more modern flavor and a new, two-color design, this sixth edition deals with principles and techniques of quantitative analysis. Examples of analytical techniques are drawn from such areas as life sciences, clinical chemistry, air and water pollution, and industrial analyses. New to this edition: Excel spreadsheets on CD-ROM * New chapters on good laboratory practice, as well as genomics and proteomics * A more modern flavor. |
Dall'interno del libro
Risultati 1-3 di 83
Pagina 358
... potential . ( But Zn2 + is a poor oxidizing agent . ) The electrode potential for Sn4 + + 2e Sn2 + is +0.15 V. In other words , the potential of this half - reaction relative to the NHE in a cell like that in Fig- ure 12.1 would be 0.15 ...
... potential . ( But Zn2 + is a poor oxidizing agent . ) The electrode potential for Sn4 + + 2e Sn2 + is +0.15 V. In other words , the potential of this half - reaction relative to the NHE in a cell like that in Fig- ure 12.1 would be 0.15 ...
Pagina 362
Gary D. Christian. This calculated potential is the potential an electrode would adopt , relative to the NHE , if it were placed in the solution , and it is a measure of the oxidizing or re- ducing power of that solution . Theoretically ...
Gary D. Christian. This calculated potential is the potential an electrode would adopt , relative to the NHE , if it were placed in the solution , and it is a measure of the oxidizing or re- ducing power of that solution . Theoretically ...
Pagina 365
... potential of a half - reaction may depend on the condi- tions of the solution . For example , the Eo value for Ce1 + + e ̄ Ce3 + is 1.61 V. However , we can change this potential by changing the acid used to acidify the so- lution ...
... potential of a half - reaction may depend on the condi- tions of the solution . For example , the Eo value for Ce1 + + e ̄ Ce3 + is 1.61 V. However , we can change this potential by changing the acid used to acidify the so- lution ...
Sommario
Chapter | 1 |
The use of spreadsheets for plotting curves and perform Least squares equation | 3 |
Chapter | 8 |
Copyright | |
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absorbance absorption acetic acid acid solution activity coefficients AgCl agent amount analysis Analytical Chemistry atomic balance base buffer buret Ca2+ calcium Calculate the pH calibration cell centration Chapter chelate Chem chemical chloride chromatography color column complex concentration detector determined dilute dissociation dissolved EDTA electrolyte end point equal Equation equilibrium constant equivalence point error example f wt Fe2+ filter flask formula weight glass gravimetric half-reaction HOAc hydrogen ion hydroxide indicator ion-selective electrode ionic strength ionization iron(III laboratory liquid measurements membrane metal ion method millimoles mmol mmol/mL molarity molecules moles NaOH Nernst equation oxidizing pipet plot potassium potential precipitate prepared proton radiation ratio react reaction reagent redox reference electrode salt sample silver sodium sodium hydroxide solubility solvent species spreadsheet standard deviation substance temperature tion titration curve volume volumetric wavelength weak acid