Analytical ChemistryXerox College Pub., 1971 - 508 pagine |
Dall'interno del libro
Risultati 1-3 di 90
Pagina 204
... Preparation of standard acid and standard base solutions . The normality of the standard HCl and standard NaOH needs to be known only to three significant figures . If you have prepared standard HCl or NaOH in Experiment 13.1 or 13.2 ...
... Preparation of standard acid and standard base solutions . The normality of the standard HCl and standard NaOH needs to be known only to three significant figures . If you have prepared standard HCl or NaOH in Experiment 13.1 or 13.2 ...
Pagina 217
... preparation of exactly 0.1000 M AgNO3 , in order that the student may obtain practice at weighing exact quantities . At the instructor's discretion , an approxi- mately 0.1 M solution may be prepared by weighing accurately about 8.5 g ...
... preparation of exactly 0.1000 M AgNO3 , in order that the student may obtain practice at weighing exact quantities . At the instructor's discretion , an approxi- mately 0.1 M solution may be prepared by weighing accurately about 8.5 g ...
Pagina 221
... prepared indicator may be used to guard against instability . This is prepared by grinding together 50 mg indicator , 5 g NaCl , and 5 g hydroxylamine hydrochloride . A small scoopful of this is added to the sample to be titrated . 17 ...
... prepared indicator may be used to guard against instability . This is prepared by grinding together 50 mg indicator , 5 g NaCl , and 5 g hydroxylamine hydrochloride . A small scoopful of this is added to the sample to be titrated . 17 ...
Sommario
Introduction | 3 |
Basic Tools of Analytical Chemistry | 15 |
Experiment | 16 |
Copyright | |
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absorbance absorption acetic acid solution activity activity coefficient added agent alkaline amount analysis analytical anion atomic beaker beta particles blood buffer buret calcium Calculate calibration carbon cathode cell chelate chloride chromatography color column complex compounds concentration constant containing coulometric crucible decrease detector determined dilute dissolved distilled water EDTA electrode electrolyte eluted end point enzyme Equation equivalence point Erlenmeyer flask error example extraction Figure filter flame flask glass glucose half-reaction hydrochloric acid hydrogen hydroxide indicator instrument iodide ion-selective electrodes ionization measured mercury metal mixture mmoles molecule NaOH Nernst equation nitrogen oxidizing oxidizing agent particles percent perchloric acid pipet potassium potential precipitate prepared procedure protein reaction reagent redox reduced salt sample separation serum sodium soluble solvent substance sulfuric sulfuric acid temperature titration titration curve tube unknown volume volumetric volumetric flask wavelength weight zero