Analytical Chemistry: An IntroductionHolt, Rinehart and Winston, 1965 - 527 pagine |
Dall'interno del libro
Risultati 1-3 di 25
Pagina 391
... iodide solution is slow , particularly where the iodide concentration is low . Because of this , it is common practice to dissolve the solid completely in a few milliliters of a very concentrated iodide solution before diluting to the ...
... iodide solution is slow , particularly where the iodide concentration is low . Because of this , it is common practice to dissolve the solid completely in a few milliliters of a very concentrated iodide solution before diluting to the ...
Pagina 392
... iodide couple since hydrogen ions do not participate in the half reaction . Many of the substances that react with iodine , however , evolve hydrogen ions in their oxidation ; the position of equilibrium may therefore be markedly ...
... iodide couple since hydrogen ions do not participate in the half reaction . Many of the substances that react with iodine , however , evolve hydrogen ions in their oxidation ; the position of equilibrium may therefore be markedly ...
Pagina 400
... iodide ion ; this can then be titrated with the solution to be standardized . Potassium Iodate . Iodate ion reacts rapidly with iodide in slightly acid solution to give iodine . 103 + 51− + 6H + ⇒ 311⁄2 + 3H2O Each formula weight of ...
... iodide ion ; this can then be titrated with the solution to be standardized . Potassium Iodate . Iodate ion reacts rapidly with iodide in slightly acid solution to give iodine . 103 + 51− + 6H + ⇒ 311⁄2 + 3H2O Each formula weight of ...
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