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 77
Pagina 280
... first equivalence point , there remains a solution of HCO3 , and [ H + ] ≈ √KalKa2 . Beyond the first equivalence point , the HCO3 is partially converted to H2CO3 ( CO2 ) and a second buffer region is established , the pH being ...
... first equivalence point , there remains a solution of HCO3 , and [ H + ] ≈ √KalKa2 . Beyond the first equivalence point , the HCO3 is partially converted to H2CO3 ( CO2 ) and a second buffer region is established , the pH being ...
Pagina 285
... first ionization constant of sulfurous acid , H2SO3 , is 1.3 × 10-2 , and the second ionization constant is 5 x 10-6 . Therefore , in a mixture with HCl , the first proton of H2SO , would titrate along with the HCl , and the pH at the ...
... first ionization constant of sulfurous acid , H2SO3 , is 1.3 × 10-2 , and the second ionization constant is 5 x 10-6 . Therefore , in a mixture with HCl , the first proton of H2SO , would titrate along with the HCl , and the pH at the ...
Pagina 644
... first - order reaction and its rate depends only on the concentration of A. Equation 22.2 is known as the differential form of the first - order rate law . The integrated form of the equation is log [ A ] = log [ A ] o - kt 2.303 ( 22.3 ) ...
... first - order reaction and its rate depends only on the concentration of A. Equation 22.2 is known as the differential form of the first - order rate law . The integrated form of the equation is log [ A ] = log [ A ] o - kt 2.303 ( 22.3 ) ...
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