Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 91
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 , H3O * , is the conjugate acid of the base ...
... 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 , H3O * , is the conjugate acid of the base ...
Pagina 193
... BASE WITH A STRONG ACID An analogous situation exists for the titration of strong bases with strong acids . In the region short of the equivalence ... BASE PAIRS Titration 193 Acids Bases Weak Titration Curves for Weak Acids or Weak Bases.
... BASE WITH A STRONG ACID An analogous situation exists for the titration of strong bases with strong acids . In the region short of the equivalence ... BASE PAIRS Titration 193 Acids Bases Weak Titration Curves for Weak Acids or Weak Bases.
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 | 58 |
Copyright | |
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absorbance absorption acid solution activity coefficient addition AgNO3 aliquot analysis analyte anode application aqueous base buffer cadmium calcium carbonate cathode cation cell cerium(IV chemical color complex concen coulometric determined dilute dissociation constant dissolved EDTA electrode potential electrolyte employed end point Equation equilibrium constant equivalence point equivalent weight error example excess Fe² Fe³ filter flask formal concentration formation formula weight glass gravimetric H₂O H3O+ half-cell half-reaction hydrogen ion hydroxide iodide iodine ionic strength iron(II K₁ liquid measurement membrane mercury(II metal method molar NaOH oxalate oxidation oxidation-reduction particles permanganate polarographic potassium precipitate primary standard quantity radiation react reactants reaction reagent reduced sample saturated silver chloride silver ion silver nitrate sodium solid solubility solution containing species standard electrode potential standard hydrogen electrode standard solution substance sulfuric acid Table temperature thiosulfate titration curves volume volumetric wavelength zinc
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