Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 89
Pagina 6
... base called its conjugate base , and every Brønsted - Lowry base is paired with a conjugate acid . In Equation 2-1 nitrite ion is seen to be the conjugate base of nitrous acid ; the hydronium ion , H , O * , is the conjugate acid of the ...
... base called its conjugate base , and every Brønsted - Lowry base is paired with a conjugate acid . In Equation 2-1 nitrite ion is seen to be the conjugate base of nitrous acid ; the hydronium ion , H , O * , is the conjugate acid of the ...
Pagina 193
... bases with strong acids . In the region short of the equivalence point the solution is highly alkaline , the hydroxide ion concentration being numerically equal to the normality of the base . The solution is neutral at the equivalence ...
... bases with strong acids . In the region short of the equivalence point the solution is highly alkaline , the hydroxide ion concentration being numerically equal to the normality of the base . The solution is neutral at the equivalence ...
Pagina 240
... base . Alternatively , the acid may be dissolved in an excess of standard base ; the unreacted base is then back - titrated with standard acid . Sulfonic acids are generally strong acids and readily dissolve in water . Their titration with ...
... base . Alternatively , the acid may be dissolved in an excess of standard base ; the unreacted base is then back - titrated with standard acid . Sulfonic acids are generally strong acids and readily dissolve in water . Their titration with ...
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