Analytical Chemistry, Volume 4Wiley, 2003 - 828 pagine This text is designed for the undergraduate one-term Quantitative Analysis course (sometimes called Analytical Chemistry) for students majoring in Chemistry and related fields. It 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.The Sixth Edition is extensively revised and updated with a more modern flavor and a new, two-color design. |
Dall'interno del libro
Risultati 1-3 di 78
Pagina 160
... agent with a reducing agent , or vice versa . An oxidizing agent gains electrons and a reducing agent loses electrons in a reaction between them . There must be a sufficiently large difference between the oxidizing and re- ducing ...
... agent with a reducing agent , or vice versa . An oxidizing agent gains electrons and a reducing agent loses electrons in a reaction between them . There must be a sufficiently large difference between the oxidizing and re- ducing ...
Pagina 297
... Agent for Metals . Simple complexing agents such as ammonia are rarely used as titrating agents be- cause a sharp ... agent that has two or more groups capable of complexing with a metal ion is called a chelating agent . The complex ...
... Agent for Metals . Simple complexing agents such as ammonia are rarely used as titrating agents be- cause a sharp ... agent that has two or more groups capable of complexing with a metal ion is called a chelating agent . The complex ...
Pagina 358
... agent . ) Zn is a good reducing agent because of the low reduction 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 ...
... agent . ) Zn is a good reducing agent because of the low reduction 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 ...
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 H₂O half-reaction HCO3 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