Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 93
Pagina 11
... concentration of Cl , CCOOH is given by MHA = [ HA ] = X ( 285 × 0.27 ) mg HA 1 = 0.047 mmole / ml 163 mg HA / mole 10.0 ml The molarity of H3O + as well as C1 , CCOO ̄ will be equal to the formal concentration of the acid minus the ...
... concentration of Cl , CCOOH is given by MHA = [ HA ] = X ( 285 × 0.27 ) mg HA 1 = 0.047 mmole / ml 163 mg HA / mole 10.0 ml The molarity of H3O + as well as C1 , CCOO ̄ will be equal to the formal concentration of the acid minus the ...
Pagina 101
... concentration at 3.4 × 10-11 mole / liter , the Fe3 + concentration will be lowered to 1.0 x 10 mole / liter . Note that quantitative precipitation of Fe ( OH ) , is achieved in a distinctly acidic solution . We must now consider ...
... concentration at 3.4 × 10-11 mole / liter , the Fe3 + concentration will be lowered to 1.0 x 10 mole / liter . Note that quantitative precipitation of Fe ( OH ) , is achieved in a distinctly acidic solution . We must now consider ...
Pagina 146
... CONCENTRATION CHANGES DURING TITRATION End points are the result of marked changes in at least one reactant concentration during the titration . For most ( but not all ) end points , changes that occur in the region surrounding the ...
... CONCENTRATION CHANGES DURING TITRATION End points are the result of marked changes in at least one reactant concentration during the titration . For most ( but not all ) end points , changes that occur in the region surrounding the ...
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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