Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 84
Pagina 195
... amount equal to [ OH ̄ ] . Thus the molar concentration of HA is given by - [ HA ] = FHA - [ H3O * ] + [ OH ̄ ] ( 9-3 ) Similarly , the reaction in Equation 9-1 increases [ A ̄ ] by an amount equal to [ H3O + ] , whereas reaction 9-2 ...
... amount equal to [ OH ̄ ] . Thus the molar concentration of HA is given by - [ HA ] = FHA - [ H3O * ] + [ OH ̄ ] ( 9-3 ) Similarly , the reaction in Equation 9-1 increases [ A ̄ ] by an amount equal to [ H3O + ] , whereas reaction 9-2 ...
Pagina 229
... amount of carbonic acid and a small amount of unreacted hydrogen carbonate . Boiling effectively destroys this buffer by eliminating the carbonic acid : H2CO3 → CO2 ( g ) + H2O As a result , the solution again acquires an alkaline pH ...
... amount of carbonic acid and a small amount of unreacted hydrogen carbonate . Boiling effectively destroys this buffer by eliminating the carbonic acid : H2CO3 → CO2 ( g ) + H2O As a result , the solution again acquires an alkaline pH ...
Pagina 251
... amount of base required for complete solution . Under normal atmospheric conditions the dihydrate Na2H2Y 2H2O contains 0.3 % moisture in excess of the stoichiometric amount . For all but the most exacting work this excess is ...
... amount of base required for complete solution . Under normal atmospheric conditions the dihydrate Na2H2Y 2H2O contains 0.3 % moisture in excess of the stoichiometric amount . For all but the most exacting work this excess is ...
Sommario
Introduction | 1 |
A Review of Simple Equilibrium Constant | 24 |
The Evaluation of Analytical Data | 58 |
Copyright | |
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absorbance absorption acid solution activity coefficient addition AgNO3 aliquot analysis analyte anode application aqueous base buffer cadmium calcium carbonate cathode cation cell cerium(IV chemical color complex concen coulometric determined dilute dissociation constant dissolved EDTA electrode potential electrolyte employed end point Equation equilibrium constant equivalence point equivalent weight error example excess Fe² Fe³ filter flask formal concentration formation formula weight glass gravimetric H₂O H3O+ half-cell half-reaction hydrogen ion hydroxide iodide iodine ionic strength iron(II K₁ liquid measurement membrane mercury(II metal method molar NaOH oxalate oxidation oxidation-reduction particles permanganate polarographic potassium precipitate primary standard quantity radiation react reactants reaction reagent reduced sample saturated silver chloride silver ion silver nitrate sodium solid solubility solution containing species standard electrode potential standard hydrogen electrode standard solution substance sulfuric acid Table temperature thiosulfate titration curves volume volumetric wavelength zinc
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