Fundamentals of Analytical ChemistryHolt, Rinehart and Winston, 1969 - 835 pagine |
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Risultati 1-3 di 87
Pagina viii
... Titration Curves , 203 Volumetric Calculations , 206 10 / Precipitation Titrations , 220 Titration Curves for Precipitation Reactions , 220 End - Point Detection , 224 Applications of Precipitation - Titration Analysis , 231 ...
... Titration Curves , 203 Volumetric Calculations , 206 10 / Precipitation Titrations , 220 Titration Curves for Precipitation Reactions , 220 End - Point Detection , 224 Applications of Precipitation - Titration Analysis , 231 ...
Pagina 359
... Titration of the excess nickel ion required 6.43 ml of standard 0.0120 F EDTA . Calculate the percentage of KCN in the sample if 31.30 ml of the EDTA solution were needed for titration of 44.60 ml of the nickel solution . 9. The ...
... Titration of the excess nickel ion required 6.43 ml of standard 0.0120 F EDTA . Calculate the percentage of KCN in the sample if 31.30 ml of the EDTA solution were needed for titration of 44.60 ml of the nickel solution . 9. The ...
Pagina 575
... complete , a conductometric analysis can be employed successfully for titrations based upon relatively unfavorable equilibria . The conductometric end point is completely nonspecific . Although the Titration Curves 575 Titration Curves,
... complete , a conductometric analysis can be employed successfully for titrations based upon relatively unfavorable equilibria . The conductometric end point is completely nonspecific . Although the Titration Curves 575 Titration Curves,
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