Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 91
Pagina 146
... Table 7-1 contains data that show the changes in hydronium ion concentration that occur when 50.00 ml of 0.1000 - F hydrochloric acid are titrated with stan- dard 0.1000 - F NaOH . To emphasize the relative changes in concentration that ...
... Table 7-1 contains data that show the changes in hydronium ion concentration that occur when 50.00 ml of 0.1000 - F hydrochloric acid are titrated with stan- dard 0.1000 - F NaOH . To emphasize the relative changes in concentration that ...
Pagina 282
... Table 12-1 ; a more comprehensive table is found in Appendix 6. In these tabulations the species in the upper left - hand part of the table are most easily reduced , as indicated by the large positive E ° values ; they are therefore the ...
... Table 12-1 ; a more comprehensive table is found in Appendix 6. In these tabulations the species in the upper left - hand part of the table are most easily reduced , as indicated by the large positive E ° values ; they are therefore the ...
Pagina 647
... table of logarithms such as that found inside the back cover . The first column of this table , labeled n , gives the first two digits of the number whose log is being sought ; the row at the top of the table gives the third digit ...
... table of logarithms such as that found inside the back cover . The first column of this table , labeled n , gives the first two digits of the number whose log is being sought ; the row at the top of the table gives the third digit ...
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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