Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 59
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 log 2 [ H + ] 2 / [ H + ] 2 PH , / ( PH ) ) = E ° 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 ...
... half - reaction in the third example E = E ° . 0.0591 log 2 [ H + ] 2 / [ H + ] 2 PH , / ( PH ) ) = E ° 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 ...
Sommario
Introduction | 1 |
A Review of Simple Equilibrium Constant | 24 |
The Evaluation of Analytical Data | 46 |
Copyright | |
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absorbance absorption acid solution activity coefficient addition AgNO3 aliquot analysis analyte anode application approximately atoms base buffer buret calcium Calculate carbonate cathode cations cell cerium(IV chemical color column complex concen copper(II coulometric crucible determined dilute dissociation constant dissolved EDTA electrode potential electrolyte employed end point Equation equilibrium constant equivalence point equivalent weight example excess filter formal concentration formation formula weight glass H₂O H3O+ half-cell half-reaction hydrogen hydronium ion hydroxide indicator iodide iodine ion concentration iron(III liquid liter measurements mercury(II metal method molar NaOH oxalate oxidation particles permanganate pipet potassium precipitate prepared primary standard Procedure quantity radiation reaction reagent reduced sample silver chloride silver ion silver nitrate sodium solid solubility solution containing solvent species standard hydrogen electrode standard solution substance sulfuric acid Table temperature thiosulfate titration curve volume volumetric flask wavelength
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