Fundamentals of Analytical ChemistryHolt, Rinehart and Winston, 1969 - 835 pagine |
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Pagina 224
... complete reaction . The poorest break is observed for the reaction that is least complete - that is , in the titration of bromate ion . Those reactions that produce silver salts having solubili- ties intermediate between these extremes ...
... complete reaction . The poorest break is observed for the reaction that is least complete - that is , in the titration of bromate ion . Those reactions that produce silver salts having solubili- ties intermediate between these extremes ...
Pagina 447
... complete with lowered acidity , care must be taken to avoid hydrolysis of the iodine that tends to occur in alkaline solutions : 12+ OH HOI + I- The hypoiodite that first forms may disproportionate in part to iodate and iodide , as ...
... complete with lowered acidity , care must be taken to avoid hydrolysis of the iodine that tends to occur in alkaline solutions : 12+ OH HOI + I- The hypoiodite that first forms may disproportionate in part to iodate and iodide , as ...
Pagina 468
... complete , the residual arsenite is titrated with a standard iodine solution . This procedure suffers from the disadvantage of requiring two standard solutions . Periodate solutions may also be standardized by adding an excess of iodide ...
... complete , the residual arsenite is titrated with a standard iodine solution . This procedure suffers from the disadvantage of requiring two standard solutions . Periodate solutions may also be standardized by adding an excess of iodide ...
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