Analytical ChemistryWiley, 6 gen 1994 - 840 pagine Extensively revised and updated, this edition is concerned primarily with quantitative analysis techniques. Describes how to design an analytical method, how to obtain a laboratory sample that is representative of the whole and to prepare it for analysis, what measurement tools are available, automated analyses and the statistical significance of the analysis. New and expanded topics include heterogeneous equilibria, diode array spectrometers, fiber-optic sensors and solid-phase extraction. |
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Pagina 135
... Activities are important in potentiometric measure- ments . See Chapter 11 . a ; = Cif ; ( 4.17 ) For ionic strengths less than 10-4 , activity coeffi- cients 4.15 ACTIVITY AND ACTIVITY COEFFICIENTS 135 Activity and Activity Coefficients.
... Activities are important in potentiometric measure- ments . See Chapter 11 . a ; = Cif ; ( 4.17 ) For ionic strengths less than 10-4 , activity coeffi- cients 4.15 ACTIVITY AND ACTIVITY COEFFICIENTS 135 Activity and Activity Coefficients.
Pagina 136
... activity coefficient . The concentration is usually expressed as molarity , and the activity has the same units as the concentration . The activity coefficient is dimensionless , but numerical values for activity coefficients do depend ...
... activity coefficient . The concentration is usually expressed as molarity , and the activity has the same units as the concentration . The activity coefficient is dimensionless , but numerical values for activity coefficients do depend ...
Pagina 139
... activity coefficients compared to 0.002 M K2SO4 , especially for the So2- ion . For higher ionic strengths , a number of empirical equations have been devel- oped . Perhaps one of the more useful is the Davies modification ( see ...
... activity coefficients compared to 0.002 M K2SO4 , especially for the So2- ion . For higher ionic strengths , a number of empirical equations have been devel- oped . Perhaps one of the more useful is the Davies modification ( see ...
Sommario
Data Handling | 14 |
Stoichiometric Calculations | 65 |
General Concepts of Equilibrium | 115 |
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absorbance acetic acid acid solution added AgCl agent analysis analyte anion base beaker buffer buret Ca2+ calcium Calculate calibration curve carbon cell Chapter chelate Chem chemical chloride chromatography color column complex compounds concentration containing detector determined dilute dissociation dissolved EDTA eluted end point enzyme Equation equilibrium constant equivalence point error example extraction Fe2+ Figure filter flame fluorescence glass H₂O half-reaction HOAc hydrogen indicator injected instrument ion-selective electrodes ionic strength ionization iron(III liquid measurements method millimoles mixture mmol mmol/mL molarity molecules moles NaOH Nernst equation obtained oxidizing oxidizing agent peak phase pipet potassium potential precipitate prepared proton quantitative radiation ratio react reaction reagent redox reference electrode salt sample separation serum silver sodium sodium hydroxide solubility solvent species spectrometry substances temperature tion titration titration curve tube unknown volume volumetric flask wavelength weak acid weight