Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 49
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 E ° 0.151 V where Agl ( s ) + e Ag + I ̃ ̄ = - Eo = +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 E ° 0.151 V where Agl ( s ) + e Ag + I ̃ ̄ = - Eo = +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 | 58 |
Copyright | |
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absorbance absorption acid solution activity coefficient addition AgNO3 aliquot analysis analyte anode application aqueous base buffer cadmium calcium carbonate cathode cation cell cerium(IV chemical color complex concen coulometric determined dilute dissociation constant dissolved EDTA electrode potential electrolyte employed end point Equation equilibrium constant equivalence point equivalent weight error example excess Fe² Fe³ filter flask formal concentration formation formula weight glass gravimetric H₂O H3O+ half-cell half-reaction hydrogen ion hydroxide iodide iodine ionic strength iron(II K₁ liquid measurement membrane mercury(II metal method molar NaOH oxalate oxidation oxidation-reduction particles permanganate polarographic potassium precipitate primary standard quantity radiation react reactants reaction reagent reduced sample saturated silver chloride silver ion silver nitrate sodium solid solubility solution containing species standard electrode potential standard hydrogen electrode standard solution substance sulfuric acid Table temperature thiosulfate titration curves volume volumetric wavelength zinc
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