Fundamentals of Analytical ChemistryHolt, Rinehart and Winston, 1969 - 835 pagine |
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Pagina 327
... solvent molecules HCOOH compete with base molecules B for a stoichiometrically limited number of hydrogen ions H + ... solvent . Thus , the equilibrium constant , K , for the reaction C , H , NH , + HOAc = C , H , NHẸ + OAc- is ...
... solvent molecules HCOOH compete with base molecules B for a stoichiometrically limited number of hydrogen ions H + ... solvent . Thus , the equilibrium constant , K , for the reaction C , H , NH , + HOAc = C , H , NHẸ + OAc- is ...
Pagina 328
... solvent . To com- plete this discussion , we must now consider the dielectric behavior of the solvent , which also influences the strengths of solute acids or bases . The dielectric constant of a solvent measures its capacity for ...
... solvent . To com- plete this discussion , we must now consider the dielectric behavior of the solvent , which also influences the strengths of solute acids or bases . The dielectric constant of a solvent measures its capacity for ...
Pagina 329
... solvent . Thus , the most ad- vantageous choice of solvent for a given titration hinges upon three interrelated properties : 1. Its autoprotolysis constant , a solvent with a low constant being desirable . 2. Its properties as a proton ...
... solvent . Thus , the most ad- vantageous choice of solvent for a given titration hinges upon three interrelated properties : 1. Its autoprotolysis constant , a solvent with a low constant being desirable . 2. Its properties as a proton ...
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