Fundamentals of Analytical ChemistryHolt, Rinehart and Winston, 1963 - 786 pagine |
Dall'interno del libro
Risultati 1-3 di 70
Pagina 381
... potential may be defined as the potential of a half - cell reaction versus the standard hydrogen electrode when the reactants and products are at unit activity . The standard electrode potential for a half - cell reaction is a ...
... potential may be defined as the potential of a half - cell reaction versus the standard hydrogen electrode when the reactants and products are at unit activity . The standard electrode potential for a half - cell reaction is a ...
Pagina 394
... potentials . A somewhat analogous effect is encountered in the behavior of the potential of the ferric - ferrous couple . As mentioned earlier , an equiformal mixture of these two ions in 1 F perchloric acid exhibits a reduction potential ...
... potentials . A somewhat analogous effect is encountered in the behavior of the potential of the ferric - ferrous couple . As mentioned earlier , an equiformal mixture of these two ions in 1 F perchloric acid exhibits a reduction potential ...
Pagina 533
... potential , beginning with values sufficiently high to ensure a reasonable current flow ; as concentration polarization sets in , the applied potential is then continuously reduced in such a manner as to keep the cathode potential at ...
... potential , beginning with values sufficiently high to ensure a reasonable current flow ; as concentration polarization sets in , the applied potential is then continuously reduced in such a manner as to keep the cathode potential at ...
Sommario
The Scope of Analytical Chemistry | 3 |
Some Elementary Concepts Important | 10 |
The Evaluation of Analytical Data | 33 |
Copyright | |
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2H₂O absorbance absorption acid solution addition analysis analytical anode application aqueous barium base buffer Calculate carbonate cathode cell Chem chemical chemist colloidal color complete compounds coprecipitation coulometric crucible determined dilute dissociation dissociation constant dissolved electrode electrolyte employed end point equation equilibrium constant equivalence point equivalent weight error example excess F solution ferric ferrous filter flask formal concentration formation formula weight grams gravimetric H₂O H₂SO half reaction hydrochloric acid hydroxide indicator iodide iodine liquid measurement metal method mixture mol/liter NaOH obtained occurs oxalate oxidation particles percent permanganate polarographic potassium precipitate procedure quantity radiation reagent reduced result salt sample saturated calomel electrode silver chloride silver ion silver nitrate sodium solid solubility solvent species standard hydrogen electrode standard solution substance sulfate sulfuric sulfuric acid surface Table temperature tion titration curve volt volts volume volumetric weak acid zinc
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