Fundamentals of Analytical ChemistryHolt, Rinehart and Winston, 1969 - 835 pagine |
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Pagina 446
... iodide complex I1⁄2 + I ̄ = Iz K = 7.1 X 102 Advantage is taken of this reaction in preparing standard solutions ... iodide solution is slow , par- ticularly where the iodide concentration is low . Therefore , it is common practice to ...
... iodide complex I1⁄2 + I ̄ = Iz K = 7.1 X 102 Advantage is taken of this reaction in preparing standard solutions ... iodide solution is slow , par- ticularly where the iodide concentration is low . Therefore , it is common practice to ...
Pagina 447
... iodide by the substance being analyzed . Two variables , pH and the presence of complexing agents , are of particular importance . In acid solutions , the pH has little influence upon the reduction potential of the iodine - iodide ...
... iodide by the substance being analyzed . Two variables , pH and the presence of complexing agents , are of particular importance . In acid solutions , the pH has little influence upon the reduction potential of the iodine - iodide ...
Pagina 457
... iodide concentration is 0.1 M. Further , for periods of 10 min or less , the air oxidation of iodide ion is not appreciable in solutions as acidic as 0.4 M. Success of the titration , therefore , hinges upon control of the hydrogen ion ...
... iodide concentration is 0.1 M. Further , for periods of 10 min or less , the air oxidation of iodide ion is not appreciable in solutions as acidic as 0.4 M. Success of the titration , therefore , hinges upon control of the hydrogen ion ...
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