Fundamentals of Analytical ChemistryHolt, Rinehart, and Winston, 1976 - 804 pagine |
Dall'interno del libro
Risultati 1-3 di 81
Pagina 184
... excess Ag + follow- ing : BH4 + 8Ag + + 80H8Ag ( s ) + H2BO3 + 5H20 Titration of excess Cl- follow- ing hydrohalogenation Precipitation of K + with known excess of B ( C6H5 ) 4 ̄ , addi- tion of excess Ag + which precipitates AgB ( C6H5 ) ...
... excess Ag + follow- ing : BH4 + 8Ag + + 80H8Ag ( s ) + H2BO3 + 5H20 Titration of excess Cl- follow- ing hydrohalogenation Precipitation of K + with known excess of B ( C6H5 ) 4 ̄ , addi- tion of excess Ag + which precipitates AgB ( C6H5 ) ...
Pagina 371
... excess iron ( II ) was back - titrated with 13.3 ml of 0.0836- / Ce4 + . Calculate the percentage of KCIO3 in the sample . The antimony ( III ) in a 1.080 - g stibnite sample required a 41.6 - ml titration with 0.0653 - N 12. Express ...
... excess iron ( II ) was back - titrated with 13.3 ml of 0.0836- / Ce4 + . Calculate the percentage of KCIO3 in the sample . The antimony ( III ) in a 1.080 - g stibnite sample required a 41.6 - ml titration with 0.0653 - N 12. Express ...
Pagina 374
... excess of Br2 to oxidize the iodide present to 103 and destroy the excess thiosulfate ion . The solution was boiled to remove the bromine , and an excess of iodide was added . The liberated iodine was titrated with 13.7 ml of 0.0352 ...
... excess of Br2 to oxidize the iodide present to 103 and destroy the excess thiosulfate ion . The solution was boiled to remove the bromine , and an excess of iodide was added . The liberated iodine was titrated with 13.7 ml of 0.0352 ...
Sommario
INTRODUCTION | 1 |
A REVIEW OF SIMPLE EQUILIBRIUMCONSTANT | 22 |
vi | 42 |
Copyright | |
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Parole e frasi comuni
absorbance absorption acetic acid acid solution addition AgNO3 aliquot analysis analytical anode application aqueous solution base Beer's law buffer calcium Calculate carbonate cathode cations Cd2+ cell cerium chemical chloride color column complex compounds copper coulometric crucible Cu2+ determined dilute dissociation dissolved EDTA electrode potential electrolyte employed end point Equation equilibrium constant equivalence point equivalent weight error ethanol example excess Fe2+ Fe3+ Figure filter flask formation formula weight glass gravimetric H₂O H3O+ half-reaction hydrochloric acid hydrogen ion hydronium ion hydroxide indicator iodide iodine ion concentration iron(III liquid measurement metal method mixture NaOH ordinarily oxalate oxidation particles perchloric acid potassium precipitate quantity radiation reactant reaction reagent reduced sample silver silver chloride sodium solid solubility solution containing solvent species standard hydrogen electrode standard solution substance sulfuric sulfuric acid temperature titration titration curve volume volumetric wavelength
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