Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
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Pagina 273
... cell shown in Figure 12-1 , the driving force for the reaction Zn ( s ) + Cu2 + Cu ( s ) + Zn2 + manifests itself as a measurable electrical force or voltage between the two electrodes . This force is the sum of two potentials called half ...
... cell shown in Figure 12-1 , the driving force for the reaction Zn ( s ) + Cu2 + Cu ( s ) + Zn2 + manifests itself as a measurable electrical force or voltage between the two electrodes . This force is the sum of two potentials called half ...
Pagina 275
... half - cell process to serve as a reference . Specifications for the standard ( or normal ) hydrogen electrode call for a hydrogen ion activity of 1.00 and a partial pressure for hydrogen of 1.00 atm . By convention the potential of the ...
... half - cell process to serve as a reference . Specifications for the standard ( or normal ) hydrogen electrode call for a hydrogen ion activity of 1.00 and a partial pressure for hydrogen of 1.00 atm . By convention the potential of the ...
Pagina 281
... half - reaction in the third example E = E ° 0.0591 2 log PH , ( PH ) ) [ H ... cell potential when the logarithmic term is zero . This condition occurs ... half - cell reaction ( versus SHE ) when all reactants and products exist at unit ...
... half - reaction in the third example E = E ° 0.0591 2 log PH , ( PH ) ) [ H ... cell potential when the logarithmic term is zero . This condition occurs ... half - cell reaction ( versus SHE ) when all reactants and products exist at unit ...
Sommario
Introduction | 1 |
A Review of Simple Equilibrium Constant | 24 |
The Evaluation of Analytical Data | 46 |
Copyright | |
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absorbance absorption activity coefficient addition AgNO3 aliquot analysis analyte anode application approximately atoms base buffer buret calcium Calculate calibration 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 zinc