Fundamentals of Analytical ChemistryHolt, Rinehart and Winston, 1963 - 786 pagine |
Dall'interno del libro
Risultati 1-3 di 35
Pagina 376
... , the electrode is said to be a standard hydrogen electrode or a normal hydrogen electrode . Quite arbitrarily the potential of this half cell is assigned the value of exactly 0 volts . Measurement of electrode potentials . Electrode ...
... , the electrode is said to be a standard hydrogen electrode or a normal hydrogen electrode . Quite arbitrarily the potential of this half cell is assigned the value of exactly 0 volts . Measurement of electrode potentials . Electrode ...
Pagina 381
... standard hydrogen electrode when the reactants and products are at unit activity . The standard electrode potential for a half - cell reaction is a fundamental physical constant that gives a quantitative description of the relative ...
... standard hydrogen electrode when the reactants and products are at unit activity . The standard electrode potential for a half - cell reaction is a fundamental physical constant that gives a quantitative description of the relative ...
Pagina 397
... hydrogen is evolved at the cathode and oxygen at the anode . The total volume of the two gases is 49.2 ml at standard conditions . 12. Calculate the reduction potentials of the following half cells against the standard hydrogen electrode ...
... hydrogen is evolved at the cathode and oxygen at the anode . The total volume of the two gases is 49.2 ml at standard conditions . 12. Calculate the reduction potentials of the following half cells against the standard hydrogen electrode ...
Sommario
The Scope of Analytical Chemistry | 3 |
Some Elementary Concepts Important | 10 |
The Evaluation of Analytical Data | 33 |
Copyright | |
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2H₂O absorbance absorption acid solution addition analysis analytical anode application aqueous barium base buffer Calculate carbonate cathode cell Chem chemical chemist colloidal color complete compounds coprecipitation coulometric crucible determined dilute dissociation dissociation constant dissolved electrode electrolyte employed end point equation equilibrium constant equivalence point equivalent weight error example excess F solution ferric ferrous filter flask formal concentration formation formula weight grams gravimetric H₂O H₂SO half reaction hydrochloric acid hydroxide indicator iodide iodine liquid measurement metal method mixture mol/liter NaOH obtained occurs oxalate oxidation particles percent permanganate polarographic potassium precipitate procedure quantity radiation reagent reduced result salt sample saturated calomel electrode silver chloride silver ion silver nitrate sodium solid solubility solvent species standard hydrogen electrode standard solution substance sulfate sulfuric sulfuric acid surface Table temperature tion titration curve volt volts volume volumetric weak acid zinc
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