Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 76
Pagina 188
... indicator equilibrium . Using HIn as an example , we may write that the indicator exhibits its pure acid color to the average observer when [ In " ] 1 [ HIn ] 10 and its basic color when ≥ [ In ̄ ] 10 [ HIn ] 1 The color appears to be ...
... indicator equilibrium . Using HIn as an example , we may write that the indicator exhibits its pure acid color to the average observer when [ In " ] 1 [ HIn ] 10 and its basic color when ≥ [ In ̄ ] 10 [ HIn ] 1 The color appears to be ...
Pagina 306
... indicator can be written as Inox + ne Inred If the indicator reaction is reversible , we may write E = Eo n 0.0591 [ Inred ] log [ Inox ] ( 12-5 ) Typically a change from the color of the oxidized form of the indicator to the reduced ...
... indicator can be written as Inox + ne Inred If the indicator reaction is reversible , we may write E = Eo n 0.0591 [ Inred ] log [ Inox ] ( 12-5 ) Typically a change from the color of the oxidized form of the indicator to the reduced ...
Pagina 583
... Indicator Solutions Discussion . Acid - base indicators exist for virtually any pH range be- tween 1 and 13.4 The theory of indicator behavior is discussed in Chapter 9 . Directions follow for the preparation of indicator solutions that ...
... Indicator Solutions Discussion . Acid - base indicators exist for virtually any pH range be- tween 1 and 13.4 The theory of indicator behavior is discussed in Chapter 9 . Directions follow for the preparation of indicator solutions that ...
Sommario
Introduction | 1 |
A Review of Simple Equilibrium Constant | 24 |
The Evaluation of Analytical Data | 46 |
Copyright | |
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absorbance absorption activity coefficient addition AgNO3 aliquot analysis analyte anode application approximately atoms base buffer buret calcium Calculate calibration carbonate cathode cations cell cerium(IV chemical color column complex concen copper(II coulometric crucible determined dilute dissociation constant dissolved EDTA electrode potential electrolyte employed end point Equation equilibrium constant equivalence point equivalent weight example excess filter formal concentration formation formula weight glass H₂O H3O+ half-cell half-reaction hydrogen hydronium ion hydroxide indicator iodide iodine ion concentration iron(III liquid liter measurements mercury(II metal method molar NaOH oxalate oxidation particles permanganate pipet potassium precipitate prepared primary standard Procedure quantity radiation reaction reagent reduced sample silver chloride silver ion silver nitrate sodium solid solubility solution containing solvent species standard hydrogen electrode standard solution substance sulfuric acid Table temperature thiosulfate titration curve volume volumetric flask wavelength zinc