Fundamentals of Analytical ChemistryHolt, Rinehart and Winston, 1969 - 835 pagine |
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Pagina 147
... mole / liter Thus , if we maintain the OH- concentration at 1.1 × 10-10 mole per liter , the Fe3 + con- centration will be 1.0 × 10-6 mole per liter . It is of interest to note that quantitative pre- cipitation of Fe ( OH ) , is ...
... mole / liter Thus , if we maintain the OH- concentration at 1.1 × 10-10 mole per liter , the Fe3 + con- centration will be 1.0 × 10-6 mole per liter . It is of interest to note that quantitative pre- cipitation of Fe ( OH ) , is ...
Pagina 255
... mole / liter pH = 4.99 In these examples we considered 1 liter of solution containing 0.1 mole of acetic acid and 0.2 mole of sodium acetate . Since the pH of a buffer is governed by the ratio between acid and salt , we would expect a ...
... mole / liter pH = 4.99 In these examples we considered 1 liter of solution containing 0.1 mole of acetic acid and 0.2 mole of sodium acetate . Since the pH of a buffer is governed by the ratio between acid and salt , we would expect a ...
Pagina 394
... mole / liter [ Fe2 + ] = 1.7 × 10-6 × 0.050 8.5 x 10-8 mole / liter Finally , the stoichiometry of the reaction requires that [ Ce1 + ] = 8.5 x 10-8 mole / liter [ Ce3 + ] = 0.050 mole / liter Now consider the somewhat more complicated ...
... mole / liter [ Fe2 + ] = 1.7 × 10-6 × 0.050 8.5 x 10-8 mole / liter Finally , the stoichiometry of the reaction requires that [ Ce1 + ] = 8.5 x 10-8 mole / liter [ Ce3 + ] = 0.050 mole / liter Now consider the somewhat more complicated ...
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