Fundamentals of Analytical ChemistrySaunders College Pub., 1988 - 894 pagine |
Dall'interno del libro
Risultati 1-3 di 95
Pagina 295
... standard electrode potential is a relative quantity in the sense that it is the potential of an electrochemical cell in which the anode is the standard hydrogen electrode , whose potential has been arbitrarily as- signed a value of zero . 2 ...
... standard electrode potential is a relative quantity in the sense that it is the potential of an electrochemical cell in which the anode is the standard hydrogen electrode , whose potential has been arbitrarily as- signed a value of zero . 2 ...
Pagina 299
... potential is then , by definition , the standard electrode potential for the half - reaction AgCl ( s ) + e Ag ( s ) + Cl- E = 0.222 V where EAgCl = 0.799 +0.0592 log Ksp = 0.222 V ( 12-4 ) 12D 12D - 1 The potential for a silver electrode ...
... potential is then , by definition , the standard electrode potential for the half - reaction AgCl ( s ) + e Ag ( s ) + Cl- E = 0.222 V where EAgCl = 0.799 +0.0592 log Ksp = 0.222 V ( 12-4 ) 12D 12D - 1 The potential for a silver electrode ...
Pagina 309
... standard electrode potentials . Henceforth , we shall use whichever is the more appropriate . Reaction Rates Standard potentials reveal ... standard electrode potential for the half - reaction 12D Applications of Electrode Potentials 309.
... standard electrode potentials . Henceforth , we shall use whichever is the more appropriate . Reaction Rates Standard potentials reveal ... standard electrode potential for the half - reaction 12D Applications of Electrode Potentials 309.
Sommario
Introduction | 1 |
Gravimetric Methods of Analysis | 57 |
Titrimetric Methods of Analysis | 84 |
Copyright | |
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absorbance absorption acetic activity coefficients addition AgNO3 aliquot analysis analytical concentration anions anode applications atoms autoprotolysis base buffer Calculate the pH carbonate cathode cations cell cell potential cerium(IV chemical chromatography color column complex compounds conjugate base coulometric Cu2+ detector determination dilute dissociation constant dissolved EDTA electrolyte end point Equation equilibrium constant equivalence point error example excess Fe2+ Fe3+ formation constant glass H₂O H3O+ half-reaction hydrogen ion hydronium ion concentration indicator iodine ionic strength iron(II KMnO4 liquid measurements membrane metal method mmol mobile phase molar concentration molecules NaOH Nernst equation obtained oxidation particles potassium precipitate quantity radiation ratio reaction reagent relative sample saturated shown in Figure silver silver chloride sodium solubility solution containing solvent species standard deviation standard electrode potentials standard hydrogen electrode standard solution Substitution Table temperature titration titration curves volume wavelength weak acid Zn2+