Analytical chemistry |
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A V/O of Precipitates From these examples it is apparent that the ionic strength of
a strong electrolyte solution consisting solely of singly charged ions is identical
with the total formal salt concentration. If the species carry multiple charges, ...
A V/O of Precipitates From these examples it is apparent that the ionic strength of
a strong electrolyte solution consisting solely of singly charged ions is identical
with the total formal salt concentration. If the species carry multiple charges, ...
Pagina
Concentration on Solubility 1 \J I At high ionic strengths the activity coefficients for
some species increase and may even become greater than one. Interpretation of
the behavior of solutions in this region is difficult; we shall confine our ...
Concentration on Solubility 1 \J I At high ionic strengths the activity coefficients for
some species increase and may even become greater than one. Interpretation of
the behavior of solutions in this region is difficult; we shall confine our ...
Pagina
Turning now to Table 5-3, we find that at an ionic strength of 0.1 = 0.38 /IO3- =
0.78 If the calculated ionic strength did not match that of one of the columns in the
table, fBj+ and /io3- could be obtained from Equation 5-27. We may thus write ...
Turning now to Table 5-3, we find that at an ionic strength of 0.1 = 0.38 /IO3- =
0.78 If the calculated ionic strength did not match that of one of the columns in the
table, fBj+ and /io3- could be obtained from Equation 5-27. We may thus write ...
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Indice
Preface v | |
Stoichiometric Relationships 15 | |
Solubility Product Constants 660 | |
Copyright | |
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absorbance absorption acid activity coefficients addition aliquot analysis application approximately atomic balance base beaker beam Beer's law bromocresol green buffer buret calcium Calculate calibration carbonate cathode cations cell cerium(IV chemical chromatography color column complex concen coulometric crucible detector determined dilute dissociation constant dissolved EDTA electrode potential electrolyte employed end point Equation equilibrium constant equivalence point equivalent weight example excess filter flame formal concentration formation formula weight glass gravimetric half-reaction heating hydrogen hydroxide indeterminate error indicator iodide iodine ionic strength iron(III liquid liter logarithm measurements metal method ml of water molar Na0H NaOH Note obtained oxalate oxidation oxidation-reduction particles permanganate pipet potassium precipitate prepared Procedure quantity radiation reaction reagent result sample silver chloride silver nitrate sodium solid solution containing solvent species standard deviation standard solution sulfuric acid Table temperature titration curve uncertainty volume volumetric flask washed wavelength
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