Fundamentals of Analytical ChemistryHolt, Rinehart and Winston, 1969 - 835 pagine |
Dall'interno del libro
Risultati 1-3 di 54
Pagina 313
... NaOH to the solution ( con- veniently 50.00 ml ) . Immediately add 10 ml of 10 percent BaCl , and 2 drops of phenolphthalein indicator . Titrate the excess NaOH at once with a standard 0.1 N HCl solution to the disappearance of the pink ...
... NaOH to the solution ( con- veniently 50.00 ml ) . Immediately add 10 ml of 10 percent BaCl , and 2 drops of phenolphthalein indicator . Titrate the excess NaOH at once with a standard 0.1 N HCl solution to the disappearance of the pink ...
Pagina 319
... NaOH would be needed to neutralize 50.0 ml of this solution ? 5. Calculate the normality of a sodium hydroxide solution on the basis of the accom- panying titration data : wt of potassium hydrogen phthalate taken , g volume of NaOH used ...
... NaOH would be needed to neutralize 50.0 ml of this solution ? 5. Calculate the normality of a sodium hydroxide solution on the basis of the accom- panying titration data : wt of potassium hydrogen phthalate taken , g volume of NaOH used ...
Pagina 322
... NaOH solution was needed to neutralize the excess acid . 33. Calculate the volume of 0.1240 F HCl needed to titrate ( a ) 26.30 ml of 0.0724 F Na , PO , to a bromcresol - green end point . ( b ) 36.1 ml of 0.1100 F Na2HPO , to a ...
... NaOH solution was needed to neutralize the excess acid . 33. Calculate the volume of 0.1240 F HCl needed to titrate ( a ) 26.30 ml of 0.0724 F Na , PO , to a bromcresol - green end point . ( b ) 36.1 ml of 0.1100 F Na2HPO , to a ...
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