Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 92
Pagina 88
... Solubility of Precipitates The solubility of a precipitate increases in the presence of ionic or molecular species that react with the ions derived from the precipitate . This effect is illustrated by the examples shown in Table 5-1 ...
... Solubility of Precipitates The solubility of a precipitate increases in the presence of ionic or molecular species that react with the ions derived from the precipitate . This effect is illustrated by the examples shown in Table 5-1 ...
Pagina 95
... solubility ( 5-13 ) Calculate the solubility of Fe ( OH ) 3 in water . As a hypothesis let us assume that the charge - balance expression simplifies to 3 [ Fe3 * ] + [ H3O + ] ≈ 3 [ Fe3 ] = [ OH- ] Substitution for [ OH- ] into the ...
... solubility ( 5-13 ) Calculate the solubility of Fe ( OH ) 3 in water . As a hypothesis let us assume that the charge - balance expression simplifies to 3 [ Fe3 * ] + [ H3O + ] ≈ 3 [ Fe3 ] = [ OH- ] Substitution for [ OH- ] into the ...
Pagina 112
... solubility of most precipitates is influenced by temperature and the presence of organic solvents . Heat is absorbed as most solids ... Solubility Additional Variables That Affect the Solubility of Precipitates Rate of Precipitate Formation.
... solubility of most precipitates is influenced by temperature and the presence of organic solvents . Heat is absorbed as most solids ... Solubility Additional Variables That Affect the Solubility of Precipitates Rate of Precipitate Formation.
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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