Fundamentals of Analytical ChemistryHolt, Rinehart and Winston, 1969 - 835 pagine |
Dall'interno del libro
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Pagina 442
... excess oxalate , and then redissolved in dilute sulfuric acid . Titration of the liberated oxalic acid required 31.53 ml of 0.1101 N KMnO4 . Calculate the percentage of calcium in the sample . Ans .: 31.15 percent Ca. 9. A 0.282 - g ...
... excess oxalate , and then redissolved in dilute sulfuric acid . Titration of the liberated oxalic acid required 31.53 ml of 0.1101 N KMnO4 . Calculate the percentage of calcium in the sample . Ans .: 31.15 percent Ca. 9. A 0.282 - g ...
Pagina 463
... excess of KI . ( b ) for standardization of a sodium hydroxide solution by titration of the protons of the acid salt . ( c ) in an iodate titration in strong HCl solution where the reduction product is ICI . 7. Each of the following ...
... excess of KI . ( b ) for standardization of a sodium hydroxide solution by titration of the protons of the acid salt . ( c ) in an iodate titration in strong HCl solution where the reduction product is ICI . 7. Each of the following ...
Pagina 481
... excess of KBr . The mixture was acidified and allowed to stand for 5 min . An excess of KI was then added and the liberated I was titrated with 17.4 ml of 0.0783 N thiosulfate . How many milligrams of acro- lein were present in the ...
... excess of KBr . The mixture was acidified and allowed to stand for 5 min . An excess of KI was then added and the liberated I was titrated with 17.4 ml of 0.0783 N thiosulfate . How many milligrams of acro- lein were present in the ...
Sommario
1 The Scope of Analytical Chemistry | 1 |
2 Review of Elementary Concepts Important to Analytical Chemistry | 7 |
3 The Evaluation of Analytical Data | 25 |
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2H₂O acetic acid acid solution addition AgNO3 aliquot analysis analytical anode aqueous autoprotolysis base buffer Calculate the pH carbonate cathode cations cell cerium(IV chemical chloride ion color complete compounds copper copper(II coulometric Cu2+ determined dilute dissolved EDTA electrode potential electrolyte employed end point equation equilibrium constant equivalence point equivalent weight error example excess F with respect filter flask formal concentration formation formula weight glass H₂O H3O+ half-cell half-reaction hydrochloric acid hydrogen ion hydroxide ion indicator iodate iodide iodine iron(II measurements mercury(II metal method mole/liter NaOH neutral oxalate percent permanganate potassium potentiometric precipitate Procedure quantity reaction reagent reducing salt sample silver ion silver nitrate sodium sodium carbonate solubility solution containing solvent species standard electrode potential standard hydrogen electrode standard solution substance sulfate sulfuric acid temperature thiosulfate tion titration titration curve volume volumetric weak acid zinc