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 acetic acid acid solution addition AgNO3 aliquot analysis analytical anode aqueous autoprotolysis base buffer Calculate the pH carbonate cathode cations cell cerium(IV chemical chloride ion color complete compounds copper copper(II coulometric Cu2+ determined dilute dissolved EDTA electrode potential electrolyte employed end point equation equilibrium constant equivalence point equivalent weight error example excess F with respect filter flask formal concentration formation formula weight glass H₂O H3O+ half-cell half-reaction hydrochloric acid hydrogen ion hydroxide ion indicator iodate iodide iodine iron(II measurements mercury(II metal method mole/liter NaOH neutral oxalate percent permanganate potassium potentiometric precipitate Procedure quantity reaction reagent reducing salt sample silver ion silver nitrate sodium sodium carbonate solubility solution containing solvent species standard electrode potential standard hydrogen electrode standard solution substance sulfate sulfuric acid temperature thiosulfate tion titration titration curve volume volumetric weak acid zinc