Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 78
Pagina 277
... electrode potential ( or more exactly , relative electrode potential ) is reserved exclusively for half - reactions written as reductions . There is no objection to the use of the term oxidation potential to connote an electrode process ...
... electrode potential ( or more exactly , relative electrode potential ) is reserved exclusively for half - reactions written as reductions . There is no objection to the use of the term oxidation potential to connote an electrode process ...
Pagina 281
... Electrode Potential , E ° . An examination of Equation 12-1 or Equation 12-2 reveals that the constant Eo is equal to the half - cell potential when the logarithmic term is zero . This condition occurs whenever the activity quotient is ...
... Electrode Potential , E ° . An examination of Equation 12-1 or Equation 12-2 reveals that the constant Eo is equal to the half - cell potential when the logarithmic term is zero . This condition occurs whenever the activity quotient is ...
Pagina 286
... potential of a silver electrode to the iodide ion concentration of a solution that is also saturated with silver iodide . When the iodide ion activity is unity , the potential is the sum of two constants ; this sum is the standard electrode ...
... potential of a silver electrode to the iodide ion concentration of a solution that is also saturated with silver iodide . When the iodide ion activity is unity , the potential is the sum of two constants ; this sum is the standard electrode ...
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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