Fundamentals of Analytical ChemistryHolt, Rinehart and Winston, 1969 - 835 pagine |
Dall'interno del libro
Risultati 1-3 di 82
Pagina 201
... equivalent to the substance with which it reacts . This condition is achieved at the equivalence point . For example , the equivalence point in the titra- tion of sodium chloride with silver nitrate is attained when exactly one formula ...
... equivalent to the substance with which it reacts . This condition is achieved at the equivalence point . For example , the equivalence point in the titra- tion of sodium chloride with silver nitrate is attained when exactly one formula ...
Pagina 222
... Equivalence point pAg and pCl . At the equivalence point , we have added an amount of silver ion identical to the amount of chloride ion in the sample ; the system here consists simply of a saturated solution of silver chloride . The ...
... Equivalence point pAg and pCl . At the equivalence point , we have added an amount of silver ion identical to the amount of chloride ion in the sample ; the system here consists simply of a saturated solution of silver chloride . The ...
Pagina 407
... equivalence point for each of the following reactions . When necessary , assume that the reactant solutions are initially 0.200 N and that the [ H + ] at the equivalence point is 0.100 M ; where appropriate , employ formal rather than ...
... equivalence point for each of the following reactions . When necessary , assume that the reactant solutions are initially 0.200 N and that the [ H + ] at the equivalence point is 0.100 M ; where appropriate , employ formal rather than ...
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