Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 23
Pagina 106
... 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 , however , the ionic strength is greater than 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 , however , the ionic strength is greater than the ...
Pagina 107
... ionic strengths ( that is , where μ < 0.1 ) . The variation of typical activity coefficients as a function of ionic strength is shown in Figure 5-3 . 2. In solutions that are not too concentrated , the activity coefficient for a given ...
... ionic strengths ( that is , where μ < 0.1 ) . The variation of typical activity coefficients as a function of ionic strength is shown in Figure 5-3 . 2. In solutions that are not too concentrated , the activity coefficient for a given ...
Pagina 111
... ionic strength of 0.1 fBa2 + = 0.38 f101 = 0.78 If the calculated ionic strength did not match that of one of the columns in the table , ƒBa2 + and f10 , - could be obtained from Equation 5-27 . We may thus write 1.57 × 10-9 ( 0.38 ) ...
... ionic strength of 0.1 fBa2 + = 0.38 f101 = 0.78 If the calculated ionic strength did not match that of one of the columns in the table , ƒBa2 + and f10 , - could be obtained from Equation 5-27 . We may thus write 1.57 × 10-9 ( 0.38 ) ...
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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