Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 76
Pagina 88
... presence of ionic or molecular species that react with the ions derived from the precipitate . This effect is illustrated by the examples shown in Table 5-1 . In the first example the solubility of barium sulfate is enhanced by the presence ...
... presence of ionic or molecular species that react with the ions derived from the precipitate . This effect is illustrated by the examples shown in Table 5-1 . In the first example the solubility of barium sulfate is enhanced by the presence ...
Pagina 337
... presence of hypoiodite in slightly alkaline solutions of iodine ( p . 333 ) , then , will seriously upset the stoichiometry of the iodine - thiosulfate reac- tion , causing too little thiosulfate or too much iodine to be used in the ...
... presence of hypoiodite in slightly alkaline solutions of iodine ( p . 333 ) , then , will seriously upset the stoichiometry of the iodine - thiosulfate reac- tion , causing too little thiosulfate or too much iodine to be used in the ...
Pagina 581
... presence of oxidizing agents because of the susceptibility of thiocyanate to attack . It is often possible to eliminate this source of interference by prior treatment of the sample with a reducing agent . The method also fails in the ...
... presence of oxidizing agents because of the susceptibility of thiocyanate to attack . It is often possible to eliminate this source of interference by prior treatment of the sample with a reducing agent . The method also fails in the ...
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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