Analytical Chemistry: An IntroductionHolt, Rinehart and Winston, 1965 - 527 pagine |
Dall'interno del libro
Risultati 1-3 di 31
Pagina 413
... potentiometric titrations . However , we must discuss in detail the determination of pH , which represents the one important application of direct potentiometry . 19.1 Methodology In a potentiometric titration a galvanic cell is formed ...
... potentiometric titrations . However , we must discuss in detail the determination of pH , which represents the one important application of direct potentiometry . 19.1 Methodology In a potentiometric titration a galvanic cell is formed ...
Pagina 439
... potentiometric measurements ; it is noteworthy that this uncertainty corresponds to a relative error in hydrogen ion concentration of about 3 percent . 6. Error in the pH of the buffer solution . Since the glass electrode must be ...
... potentiometric measurements ; it is noteworthy that this uncertainty corresponds to a relative error in hydrogen ion concentration of about 3 percent . 6. Error in the pH of the buffer solution . Since the glass electrode must be ...
Pagina 442
... potentiometric principle have come on the market . These are useful where a large number of routine analyses are to be carried out . Such instruments cannot yield more accurate results than those obtained by manual potentiometric tech ...
... potentiometric principle have come on the market . These are useful where a large number of routine analyses are to be carried out . Such instruments cannot yield more accurate results than those obtained by manual potentiometric tech ...
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