Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 46
Pagina 24
... chemist to decide whether or not a reaction is suitable for analytical purposes and to choose conditions which will minimize the error associated with an analysis . Equilibrium constant expressions are algebraic equations that relate ...
... chemist to decide whether or not a reaction is suitable for analytical purposes and to choose conditions which will minimize the error associated with an analysis . Equilibrium constant expressions are algebraic equations that relate ...
Pagina 70
... chemist ordinarily takes advantage of the relatively large gain afforded by averaging two to four measurements but can seldom afford the time required for further increases in confidence . Confidence Limits When ☛ Is Unknown ...
... chemist ordinarily takes advantage of the relatively large gain afforded by averaging two to four measurements but can seldom afford the time required for further increases in confidence . Confidence Limits When ☛ Is Unknown ...
Pagina 83
... chemist obtained the following results for the determination of sulfur in a contaminated kerosene sample : 0.300 % , 0.316 % , 0.303 % . Calculate the 95 % confidence limits for the mean of this analysis . 22. Four replicate fluoride ...
... chemist obtained the following results for the determination of sulfur in a contaminated kerosene sample : 0.300 % , 0.316 % , 0.303 % . Calculate the 95 % confidence limits for the mean of this analysis . 22. Four replicate fluoride ...
Sommario
Introduction | 1 |
A Review of Simple Equilibrium Constant | 24 |
The Evaluation of Analytical Data | 46 |
Copyright | |
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absorbance absorption activity coefficient addition AgNO3 aliquot analysis analyte anode application approximately atoms base buffer buret calcium Calculate calibration carbonate cathode cations cell cerium(IV chemical color column complex concen copper(II coulometric crucible determined dilute dissociation constant dissolved EDTA electrode potential electrolyte employed end point Equation equilibrium constant equivalence point equivalent weight example excess filter formal concentration formation formula weight glass H₂O H3O+ half-cell half-reaction hydrogen hydronium ion hydroxide indicator iodide iodine ion concentration iron(III liquid liter measurements mercury(II metal method molar NaOH oxalate oxidation particles permanganate pipet potassium precipitate prepared primary standard Procedure quantity radiation reaction reagent reduced sample silver chloride silver ion silver nitrate sodium solid solubility solution containing solvent species standard hydrogen electrode standard solution substance sulfuric acid Table temperature thiosulfate titration curve volume volumetric flask wavelength zinc