Analytical Chemistry: An IntroductionHolt, Rinehart and Winston, 1965 - 527 pagine |
Dall'interno del libro
Risultati 1-3 di 23
Pagina 320
... zinc to the copper ( II ) ions . This transfer can be expected to con- tinue until the copper ( II ) and zinc ion concentrations achieve levels corresponding to equilibrium for the reaction Zn + Cu2 + Zn2 + + Cu When this point is ...
... zinc to the copper ( II ) ions . This transfer can be expected to con- tinue until the copper ( II ) and zinc ion concentrations achieve levels corresponding to equilibrium for the reaction Zn + Cu2 + Zn2 + + Cu When this point is ...
Pagina 336
... zinc to zinc ions and reduction of the copper ( II ) ions to the metal . Standard electrode potentials for these half reactions are available ; however , these are actually potentials for cells in which the chemical reactions are Zn + ...
... zinc to zinc ions and reduction of the copper ( II ) ions to the metal . Standard electrode potentials for these half reactions are available ; however , these are actually potentials for cells in which the chemical reactions are Zn + ...
Pagina 369
... zinc as the reducing agent . Figure 18.1 illustrates a typical Jones reductor . The column is packed with granular zinc that has been amalgamated by treatment with a solution of mercury ( II ) nitrate or chloride ; metallic mercury ...
... zinc as the reducing agent . Figure 18.1 illustrates a typical Jones reductor . The column is packed with granular zinc that has been amalgamated by treatment with a solution of mercury ( II ) nitrate or chloride ; metallic mercury ...
Sommario
The Scope of Analytical Chemistry | 1 |
Some Elementary Concepts | 7 |
The Evaluation of Analytical Data | 34 |
Copyright | |
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absorbance absorption acid solution addition AgCl AgNO3 aliquot analysis analytical barium base buffer buret Calculate carbonate cell cerium chemical chemist chloride ion colloidal color complex compound coprecipitation crucible determined deviation dilute dissociation dissolved employed end point equation equilibrium constant equivalence point equivalent weight error example excess F solution Fe2+ filter flask formal concentration formula weight grams gravimetric H₂ H₂O H3O+ half reaction hydrogen ion hydronium ion hydroxide indicator iodide iodine ion concentration iron iron III KMnO4 liquid liter measurement metal method milliequivalents ml of water mol/liter NaOH normality oxalate oxidation particles percent permanganate phenolphthalein pipet potassium potentiometric precipitate quantity radiation reagent reduced result salt sample silver chloride silver ion silver nitrate sodium sodium carbonate solid solubility solvent species standard hydrogen electrode standard solution substance sulfate sulfuric acid temperature thiocyanate tion titration curve volt volume volumetric wash weak acid