Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 32
Pagina 197
... buffer solution is defined as a solution that resists changes in pH as a result of either dilution or small additions of acids or bases . The most effective buffer solution contains large and approximately equal concen- trations of a ...
... buffer solution is defined as a solution that resists changes in pH as a result of either dilution or small additions of acids or bases . The most effective buffer solution contains large and approximately equal concen- trations of a ...
Pagina 201
... buffer was only about 0.04 to 0.05 . The buffer capacity of a solution is defined as the number of equivalents of strong acid or base needed to cause 1.00 liter of the buffer to undergo a 1.00 - unit change in pH . As we have seen , the ...
... buffer was only about 0.04 to 0.05 . The buffer capacity of a solution is defined as the number of equivalents of strong acid or base needed to cause 1.00 liter of the buffer to undergo a 1.00 - unit change in pH . As we have seen , the ...
Pagina 222
... buffer that is ( c ) potassium hydrogen sulfite . ( d ) sodium hydrogen malonate . ( a ) 0.150 F in NH3 and 0.100 F in ( NH4 ) 2SO4 . ( b ) 0.0200 F in phenol and 0.0300 F in sodium phenolate . ( c ) 0.0120 F in sulfamic acid and 0.0200 ...
... buffer that is ( c ) potassium hydrogen sulfite . ( d ) sodium hydrogen malonate . ( a ) 0.150 F in NH3 and 0.100 F in ( NH4 ) 2SO4 . ( b ) 0.0200 F in phenol and 0.0300 F in sodium phenolate . ( c ) 0.0120 F in sulfamic acid and 0.0200 ...
Sommario
Introduction | 1 |
A Review of Simple Equilibrium Constant | 24 |
The Evaluation of Analytical Data | 58 |
Copyright | |
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Parole e frasi comuni
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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