Fundamentals of Analytical ChemistryHolt, Rinehart and Winston, 1969 - 835 pagine |
Dall'interno del libro
Risultati 1-3 di 79
Pagina 468
... compounds and periodate are never rapid enough to permit a direct titration . Therefore , an excess of oxidant is always used and time is allowed for the reaction to take place . Most oxidations are complete in 30 min to 1 hr at room ...
... compounds and periodate are never rapid enough to permit a direct titration . Therefore , an excess of oxidant is always used and time is allowed for the reaction to take place . Most oxidations are complete in 30 min to 1 hr at room ...
Pagina 618
... compounds containing these groups are thus subject to analysis by the polarographic technique . In general , the reactions of organic compounds at a microelectrode are slower and more complex than those of inorganic cations . Thus ...
... compounds containing these groups are thus subject to analysis by the polarographic technique . In general , the reactions of organic compounds at a microelectrode are slower and more complex than those of inorganic cations . Thus ...
Pagina 766
... compounds . Alkali - metal decompositions have proved useful for the quantitative deter- mination of the halogens in general , and fluorine in particular . Compounds of fluorine are often quite refractory toward the ordinary oxidative ...
... compounds . Alkali - metal decompositions have proved useful for the quantitative deter- mination of the halogens in general , and fluorine in particular . Compounds of fluorine are often quite refractory toward the ordinary oxidative ...
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 acetic acid acid solution addition AgNO3 aliquot analysis analytical anode aqueous autoprotolysis base buffer Calculate the pH carbonate cathode cations cell cerium(IV chemical chloride ion color complete compounds copper copper(II coulometric Cu2+ determined dilute dissolved EDTA electrode potential electrolyte employed end point equation equilibrium constant equivalence point equivalent weight error example excess F with respect filter flask formal concentration formation formula weight glass H₂O H3O+ half-cell half-reaction hydrochloric acid hydrogen ion hydroxide ion indicator iodate iodide iodine iron(II measurements mercury(II metal method mole/liter NaOH neutral oxalate percent permanganate potassium potentiometric precipitate Procedure quantity reaction reagent reducing salt sample silver ion silver nitrate sodium sodium carbonate solubility solution containing solvent species standard electrode potential standard hydrogen electrode standard solution substance sulfate sulfuric acid temperature thiosulfate tion titration titration curve volume volumetric weak acid zinc