Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 78
Pagina 5
... dissolved in them . For example , when nitrous acid is dissolved in water , the solvent acts as a proton acceptor and thus behaves as a base : ( 2-1 ) HNO2 + H2O = NO2 ̄ ̄ + H3O + acid , base2 base , acid , On the other hand , when ...
... dissolved in them . For example , when nitrous acid is dissolved in water , the solvent acts as a proton acceptor and thus behaves as a base : ( 2-1 ) HNO2 + H2O = NO2 ̄ ̄ + H3O + acid , base2 base , acid , On the other hand , when ...
Pagina 185
... dissolved in acid and treated with 50.0 ml of 0.0982 - N K4Fe ( CN ) 6 . After the formation of the solid K2Zn3 [ Fe ( CN ) 6 ] 3 was complete , the excess K4Fe ( CN ) , was back - titrated with 7.97 ml of 0.116 - N Zn2 + employing ...
... dissolved in acid and treated with 50.0 ml of 0.0982 - N K4Fe ( CN ) 6 . After the formation of the solid K2Zn3 [ Fe ( CN ) 6 ] 3 was complete , the excess K4Fe ( CN ) , was back - titrated with 7.97 ml of 0.116 - N Zn2 + employing ...
Pagina 266
... dissolved with hydrochloric acid ; the solution was then diluted to exactly 100 ml . A 25.0 - ml aliquot was buffered to pH 5 and 50.00 ml of 0.0109 - F EDTA were added . Titration of the excess chelating reagent required 8.41 ml of ...
... dissolved with hydrochloric acid ; the solution was then diluted to exactly 100 ml . A 25.0 - ml aliquot was buffered to pH 5 and 50.00 ml of 0.0109 - F EDTA were added . Titration of the excess chelating reagent required 8.41 ml of ...
Sommario
Introduction | 1 |
A Review of Simple Equilibrium Constant | 24 |
The Evaluation of Analytical Data | 46 |
Copyright | |
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absorbance absorption activity coefficient addition AgNO3 aliquot analysis analyte anode application approximately atoms base buffer buret calcium Calculate calibration carbonate cathode cations cell cerium(IV chemical color column complex concen copper(II coulometric crucible determined dilute dissociation constant dissolved EDTA electrode potential electrolyte employed end point Equation equilibrium constant equivalence point equivalent weight example excess filter formal concentration formation formula weight glass H₂O H3O+ half-cell half-reaction hydrogen hydronium ion hydroxide indicator iodide iodine ion concentration iron(III liquid liter measurements mercury(II metal method molar NaOH oxalate oxidation particles permanganate pipet potassium precipitate prepared primary standard Procedure quantity radiation reaction reagent reduced sample silver chloride silver ion silver nitrate sodium solid solubility solution containing solvent species standard hydrogen electrode standard solution substance sulfuric acid Table temperature thiosulfate titration curve volume volumetric flask wavelength zinc