Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 57
Pagina 269
... redox equilibrium constants . Separation of an oxidation - reduction reaction into its component parts ( that is , into half - reactions ) is a convenient way of indicating clearly the species that gains electrons and the one that loses ...
... redox equilibrium constants . Separation of an oxidation - reduction reaction into its component parts ( that is , into half - reactions ) is a convenient way of indicating clearly the species that gains electrons and the one that loses ...
Pagina 273
... half - reaction occurring at the anode and the other with the half - reaction taking place at the cathode . It is not difficult to see how we might obtain information regarding the relative magnitudes of half - cell potentials . For ...
... half - reaction occurring at the anode and the other with the half - reaction taking place at the cathode . It is not difficult to see how we might obtain information regarding the relative magnitudes of half - cell potentials . For ...
Pagina 281
... half - reaction in the third example E = E ° 0.0591 2 log PH , ( PH , ) [ H + ] / [ H + ] 2 = E0 2 0.0591 2 log PH2 / 1.00 [ H + ] 2 / ( 1.00 ) 2 Here ( PH ) is the partial pressure of hydrogen in its standard state , which is 1.00 atm ...
... half - reaction in the third example E = E ° 0.0591 2 log PH , ( PH , ) [ H + ] / [ H + ] 2 = E0 2 0.0591 2 log PH2 / 1.00 [ H + ] 2 / ( 1.00 ) 2 Here ( PH ) is the partial pressure of hydrogen in its standard state , which is 1.00 atm ...
Sommario
Introduction | 1 |
A Review of Simple Equilibrium Constant | 24 |
The Evaluation of Analytical Data | 58 |
Copyright | |
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absorbance absorption acid solution activity coefficient addition AgNO3 aliquot analysis analyte anode application aqueous base buffer cadmium calcium carbonate cathode cation cell cerium(IV chemical color complex concen coulometric determined dilute dissociation constant dissolved EDTA electrode potential electrolyte employed end point Equation equilibrium constant equivalence point equivalent weight error example excess Fe² Fe³ filter flask formal concentration formation formula weight glass gravimetric H₂O H3O+ half-cell half-reaction hydrogen ion hydroxide iodide iodine ionic strength iron(II K₁ liquid measurement membrane mercury(II metal method molar NaOH oxalate oxidation oxidation-reduction particles permanganate polarographic potassium precipitate primary standard quantity radiation react reactants reaction reagent reduced sample saturated silver chloride silver ion silver nitrate sodium solid solubility solution containing species standard electrode potential standard hydrogen electrode standard solution substance sulfuric acid Table temperature thiosulfate titration curves volume volumetric wavelength zinc
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