Analytical Chemistry: An IntroductionHolt, Rinehart and Winston, 1965 - 527 pagine |
Dall'interno del libro
Risultati 1-3 di 39
Pagina 328
... half reactions of zinc and cadmium , however , it becomes necessary to ... reaction opposite to that of the other two . Sign Conventions for Electrode ... reaction positive if the reaction , as written , proceeds spontaneously relative to ...
... half reactions of zinc and cadmium , however , it becomes necessary to ... reaction opposite to that of the other two . Sign Conventions for Electrode ... reaction positive if the reaction , as written , proceeds spontaneously relative to ...
Pagina 329
... half reaction , as above , beside the poten- tial of the half cell . Note also that , the sign of the electrode potential is employed here to indicate the direction of the spontaneous chemical reac- tion . This sign should not be ...
... half reaction , as above , beside the poten- tial of the half cell . Note also that , the sign of the electrode potential is employed here to indicate the direction of the spontaneous chemical reac- tion . This sign should not be ...
Pagina 337
... half reactions as written . 3. Add the potentials and the equations for the half reactions . A posi- tive cell potential will indicate that the cell reaction is spontaneous as written ; a negative sign , on the other hand , will mean ...
... half reactions as written . 3. Add the potentials and the equations for the half reactions . A posi- tive cell potential will indicate that the cell reaction is spontaneous as written ; a negative sign , on the other hand , will mean ...
Sommario
The Scope of Analytical Chemistry | 1 |
Some Elementary Concepts | 7 |
The Evaluation of Analytical Data | 34 |
Copyright | |
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absorbance absorption acid solution addition AgCl AgNO3 aliquot analysis analytical barium base buffer buret Calculate carbonate cell cerium chemical chemist chloride ion colloidal color complex compound coprecipitation crucible determined deviation dilute dissociation dissolved employed end point equation equilibrium constant equivalence point equivalent weight error example excess F solution Fe2+ filter flask formal concentration formula weight grams gravimetric H₂ H₂O H3O+ half reaction hydrogen ion hydronium ion hydroxide indicator iodide iodine ion concentration iron iron III KMnO4 liquid liter measurement metal method milliequivalents ml of water mol/liter NaOH normality oxalate oxidation particles percent permanganate phenolphthalein pipet potassium potentiometric precipitate quantity radiation reagent reduced result salt sample silver chloride silver ion silver nitrate sodium sodium carbonate solid solubility solvent species standard hydrogen electrode standard solution substance sulfate sulfuric acid temperature thiocyanate tion titration curve volt volume volumetric wash weak acid