Fundamentals of Analytical ChemistryHolt, Rinehart and Winston, 1969 - 835 pagine |
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Pagina 144
... chloride is plotted against the log of the potassium chloride concentration of the solution . At chloride con- centrations less than 10-3 F , the data found by experiment do not differ greatly from solubilities calculated from the ...
... chloride is plotted against the log of the potassium chloride concentration of the solution . At chloride con- centrations less than 10-3 F , the data found by experiment do not differ greatly from solubilities calculated from the ...
Pagina 485
... chloride and that the cells differ only with respect to the po- tassium chloride concentration . Note also that the potential of the normal calomel electrode is greater than the standard potential for the half - reaction because the ...
... chloride and that the cells differ only with respect to the po- tassium chloride concentration . Note also that the potential of the normal calomel electrode is greater than the standard potential for the half - reaction because the ...
Pagina 487
... chloride that is also satu- rated with silver chloride : AgCl ( sat'd ) , KCl ( xF ) | Ag The half - reaction is AgCl + e Ag + Cl- = E ° 0.222 V Normally , this electrode is prepared with a saturated potassium chloride solu- tion , the ...
... chloride that is also satu- rated with silver chloride : AgCl ( sat'd ) , KCl ( xF ) | Ag The half - reaction is AgCl + e Ag + Cl- = E ° 0.222 V Normally , this electrode is prepared with a saturated potassium chloride solu- tion , the ...
Sommario
1 The Scope of Analytical Chemistry | 1 |
2 Review of Elementary Concepts Important to Analytical Chemistry | 7 |
3 The Evaluation of Analytical Data | 25 |
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2H₂O absorbance absorption acetic acetic acid acid solution addition AgNO3 alkaline analysis analytical anode application aqueous base buffer calcium Calculate carbonate cathode cations cell cerium(IV chemical chloride color complex compounds copper(II coulometric crucible determined dilute dissociation dissolved EDTA electrolyte employed end point equation equilibrium constant equivalence point error ethanol example excess F with respect Fe3+ filter flask formal concentration formation glass H₂O H3O+ half-reaction hydrochloric acid hydrogen ion hydronium ion indicator iodide iodine ion concentration iron(III liquid measurement mercury(II metal method mixture mole/liter NaOH obtained oxalate oxidation particles percent perchloric acid permanganate potassium precipitate procedure quantity radiation reaction reagent reduced result salt sample saturated calomel electrode silver ion sodium solid solubility solution containing solvent species standard hydrogen electrode standard solution substance sulfate sulfuric sulfuric acid temperature tion titration titration curve volume volumetric wavelength weak acid