Analytical Chemistry: An IntroductionHolt, Rinehart and Winston, 1965 - 527 pagine |
Dall'interno del libro
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Pagina 10
... acid ) for ammonia ; the term amphi- protic is used to describe solvents that possess this dual capacity . The extent to which an acid ( or base ) reacts with a given solvent varies greatly . For example , the reaction between hydrochloric ...
... acid ) for ammonia ; the term amphi- protic is used to describe solvents that possess this dual capacity . The extent to which an acid ( or base ) reacts with a given solvent varies greatly . For example , the reaction between hydrochloric ...
Pagina 161
... acidity of the sample is therefore adjusted by the successive addition of ammonia and hydrochloric acid . Then formic acid and ammonium chloride are introduced , the former to yield the desired basic formate precipitate , and the latter ...
... acidity of the sample is therefore adjusted by the successive addition of ammonia and hydrochloric acid . Then formic acid and ammonium chloride are introduced , the former to yield the desired basic formate precipitate , and the latter ...
Pagina 297
... acid solutions are standardized in several ways . One method involves determining the anion content of the solution by a gravimetric procedure . Thus , for hydrochloric acid , a silver chloride precipitate may be used ; for sulfuric acid ...
... acid solutions are standardized in several ways . One method involves determining the anion content of the solution by a gravimetric procedure . Thus , for hydrochloric acid , a silver chloride precipitate may be used ; for sulfuric acid ...
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