Fundamentals of Analytical ChemistrySaunders College Pub., 1988 - 894 pagine |
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Risultati 1-3 di 77
Pagina 87
... Molar Concentrations The term molar M is a concentration unit that is equal to the number of moles of a solute contained in 1 L of solution or the number of millimoles of a solute in 1 mL . For example , a 0.1 M NaCl solution contains ...
... Molar Concentrations The term molar M is a concentration unit that is equal to the number of moles of a solute contained in 1 L of solution or the number of millimoles of a solute in 1 mL . For example , a 0.1 M NaCl solution contains ...
Pagina 88
... molar concentration of a particular species that exists in a solution at equilibrium . In order to state the species molarity , it is necessary to know something about the behavior of a solute when it is dissolved in a solvent . For ...
... molar concentration of a particular species that exists in a solution at equilibrium . In order to state the species molarity , it is necessary to know something about the behavior of a solute when it is dissolved in a solvent . For ...
Pagina 137
... molar species concentrations . Also , we know that the only source of ammonia - containing species is the 0.010 M ... concentration . For example , the number of moles of positive charge contributed to a solution by MgCl2 is twice the molar ...
... molar species concentrations . Also , we know that the only source of ammonia - containing species is the 0.010 M ... concentration . For example , the number of moles of positive charge contributed to a solution by MgCl2 is twice the molar ...
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