Analytical Chemistry: An IntroductionHolt, Rinehart and Winston, 1965 - 527 pagine |
Dall'interno del libro
Risultati 1-3 di 81
Pagina 20
... Equilibrium constants have been measured for a large number of chemi- cal reactions ; their values vary over a range of 10100 or more . A large value of K for an equilibrium clearly indicates that the reaction proceeds far to the right ...
... Equilibrium constants have been measured for a large number of chemi- cal reactions ; their values vary over a range of 10100 or more . A large value of K for an equilibrium clearly indicates that the reaction proceeds far to the right ...
Pagina 21
... equilibrium constants to be sure that they are applied only at the proper temperature . SOME COMMON TYPES OF EQUILIBRIUM CONSTANTS The analytical chemist is vitally concerned with chemical equilibria in aqueous solutions . Five types ...
... equilibrium constants to be sure that they are applied only at the proper temperature . SOME COMMON TYPES OF EQUILIBRIUM CONSTANTS The analytical chemist is vitally concerned with chemical equilibria in aqueous solutions . Five types ...
Pagina 338
... Equilibrium Constants from Standard Electrode Potentials An Important Condition at Equilibrium . Consider once again the galvanic cell shown in Figure 16.1 ... Equilibrium in Cells; Equilibrium Constants from Standard Electrode Potentials.
... Equilibrium Constants from Standard Electrode Potentials An Important Condition at Equilibrium . Consider once again the galvanic cell shown in Figure 16.1 ... Equilibrium in Cells; Equilibrium Constants from Standard Electrode Potentials.
Sommario
The Scope of Analytical Chemistry | 1 |
Some Elementary Concepts | 7 |
The Evaluation of Analytical Data | 34 |
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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