Fundamentals of Analytical ChemistrySaunders College Pub., 1988 - 894 pagine |
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Risultati 1-3 di 15
Pagina 105
... Autoprotolysis Amphiprotic solvents undergo self - ionization , or autoprotolysis , to form a pair of ionic species . Autoprotolysis is yet another example of an acid / base reaction , as illustrated by the following equations : base + ...
... Autoprotolysis Amphiprotic solvents undergo self - ionization , or autoprotolysis , to form a pair of ionic species . Autoprotolysis is yet another example of an acid / base reaction , as illustrated by the following equations : base + ...
Pagina 246
... autoprotolysis constant , the inherent acidity or basicity , and the dielectric constant of the solvent . The Effect of Solvent Autoprotolysis Constant In water , the titration of a weak base B with a strong acid can be formulated as B ...
... autoprotolysis constant , the inherent acidity or basicity , and the dielectric constant of the solvent . The Effect of Solvent Autoprotolysis Constant In water , the titration of a weak base B with a strong acid can be formulated as B ...
Pagina 248
... autoprotolysis constant ; a numerically small value is desirable . 2. Its properties as a proton donor or acceptor . For the titration of a weak base , a solvent with strong proton donor tendencies ( that is , an acidic solvent ) is ...
... autoprotolysis constant ; a numerically small value is desirable . 2. Its properties as a proton donor or acceptor . For the titration of a weak base , a solvent with strong proton donor tendencies ( that is , an acidic solvent ) is ...
Sommario
Introduction | 1 |
Evaluation of Analytical Data | 6 |
Gravimetric Methods of Analysis | 57 |
Copyright | |
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absorbance absorption acid activity added addition amount analysis analyte applications aqueous assume atoms base becomes buffer Calculate carbonate cations cause cell chemical chloride chromatography color column common complex compounds concentration constant containing curve derived described determination deviation difference dilute dissociation dissolved EDTA effect electrode electrode potential end point Equation equilibrium equivalence error example excess expression Figure formation given gives glass H3O+ hydrogen important increases indicator involves ion concentration less liquid mean measurements metal method mmol molar NaOH Note obtained occurs organic oxidation particles phase potential precipitate prepared present Problem quantity radiation range ratio reaction reagent reduced relative sample separation shown silver sodium solid solubility solution solvent species standard Step strong Substitution surface Table temperature titration titration curves volume weak weight