Analytical Chemistry: An IntroductionHolt, Rinehart and Winston, 1965 - 527 pagine |
Dall'interno del libro
Risultati 1-3 di 90
Pagina 122
... precipitate was washed with 200 ml of water . ( a ) Calculate the milligrams of precipitate lost by solubility in the original solution . ans . 0.58 mg ( b ) Calculate the milligrams of precipitate lost in the wash liquid . Assume that ...
... precipitate was washed with 200 ml of water . ( a ) Calculate the milligrams of precipitate lost by solubility in the original solution . ans . 0.58 mg ( b ) Calculate the milligrams of precipitate lost in the wash liquid . Assume that ...
Pagina 143
... precipitate . Another example of improving the purity of a precipitate through the judicious choice of wash liquid arises when iron is precipitated as the hydrous iron ( III ) oxide ; here , hydroxyl ions are adsorbed on the sur- face ...
... precipitate . Another example of improving the purity of a precipitate through the judicious choice of wash liquid arises when iron is precipitated as the hydrous iron ( III ) oxide ; here , hydroxyl ions are adsorbed on the sur- face ...
Pagina 214
... precipitate upon which successful indicator action depends . ( 1 ) Since this is a surface phenomenon , the precipitate should be pro- duced in a highly dispersed state ; this is one of the few instances where the analytical chemist is ...
... precipitate upon which successful indicator action depends . ( 1 ) Since this is a surface phenomenon , the precipitate should be pro- duced in a highly dispersed state ; this is one of the few instances where the analytical chemist is ...
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