Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 52
Pagina 172
... iodide ion and 0.1000 F in chloride with 0.2000 - F silver nitrate . Because silver iodide has a much smaller solubility than silver chloride , the initial additions of the reagent will result in formation of the iodide exclusively ...
... iodide ion and 0.1000 F in chloride with 0.2000 - F silver nitrate . Because silver iodide has a much smaller solubility than silver chloride , the initial additions of the reagent will result in formation of the iodide exclusively ...
Pagina 286
... iodide . When the iodide ion activity is unity , the potential is the sum of two constants ; this sum is the standard electrode potential for the half - reaction AgI ( s ) + e Ag + I E ° = -0.151 V where E ° +0.799+ 0.0591 log Ksp ...
... iodide . When the iodide ion activity is unity , the potential is the sum of two constants ; this sum is the standard electrode potential for the half - reaction AgI ( s ) + e Ag + I E ° = -0.151 V where E ° +0.799+ 0.0591 log Ksp ...
Pagina 332
... iodide solution is slow , particularly where the iodide concentration is low . As a consequence , it is necessary to dissolve the solid completely in a small amount of a concentrated iodide solution before diluting to the desired volume ...
... iodide solution is slow , particularly where the iodide concentration is low . As a consequence , it is necessary to dissolve the solid completely in a small amount of a concentrated iodide solution before diluting to the desired volume ...
Sommario
Introduction | 1 |
A Review of Simple Equilibrium Constant | 24 |
The Evaluation of Analytical Data | 46 |
Copyright | |
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absorbance absorption acid solution activity coefficient addition AgNO3 aliquot analysis analyte anode application approximately atoms base buffer buret calcium Calculate 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
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