Fundamentals of Analytical ChemistryHolt, Rinehart and Winston, 1969 - 835 pagine |
Dall'interno del libro
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Pagina 253
... buffer solution that is 0.040 F in formic acid and 0.100 F in sodium formate ; employ activities and compare the result with that obtained on page 251 . We shall assume that the ionic strength of ... Buffer Solutions 253 Buffer Solutions,
... buffer solution that is 0.040 F in formic acid and 0.100 F in sodium formate ; employ activities and compare the result with that obtained on page 251 . We shall assume that the ionic strength of ... Buffer Solutions 253 Buffer Solutions,
Pagina 255
... buffer solution after addition of 10 mfw of HCl . We may predict an increase in the concentration of undissociated acetic acid as well as a decrease in the acetate concentration , owing to the reaction between the latter and the ...
... buffer solution after addition of 10 mfw of HCl . We may predict an increase in the concentration of undissociated acetic acid as well as a decrease in the acetate concentration , owing to the reaction between the latter and the ...
Pagina 256
... buffer solution . Buffer capacity can be calculated if the composition of the buffer is known . Ordinarily , a high buffer capacity is desirable , and one obvious way of achiev- ing this is by using high reagent concentrations . Less ...
... buffer solution . Buffer capacity can be calculated if the composition of the buffer is known . Ordinarily , a high buffer capacity is desirable , and one obvious way of achiev- ing this is by using high reagent concentrations . Less ...
Sommario
1 The Scope of Analytical Chemistry | 1 |
2 Review of Elementary Concepts Important to Analytical Chemistry | 7 |
3 The Evaluation of Analytical Data | 25 |
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2H₂O absorbance absorption acetic acetic acid acid solution addition AgNO3 alkaline analysis analytical anode application aqueous base buffer calcium Calculate carbonate cathode cations cell cerium(IV chemical chloride color complex compounds copper(II coulometric crucible determined dilute dissociation dissolved EDTA electrolyte employed end point equation equilibrium constant equivalence point error ethanol example excess F with respect Fe3+ filter flask formal concentration formation glass H₂O H3O+ half-reaction hydrochloric acid hydrogen ion hydronium ion indicator iodide iodine ion concentration iron(III liquid measurement mercury(II metal method mixture mole/liter NaOH obtained oxalate oxidation particles percent perchloric acid permanganate potassium precipitate procedure quantity radiation reaction reagent reduced result salt sample saturated calomel electrode silver ion sodium solid solubility solution containing solvent species standard hydrogen electrode standard solution substance sulfate sulfuric sulfuric acid temperature tion titration titration curve volume volumetric wavelength weak acid