Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 86
Pagina 221
... Calculate the pH of a solution prepared by mixing 25.0 ml of 0.0500 - F NH3 with 25.0 ml of ( a ) water . ( b ) 0.0100 - F NaOH . ( c ) 0.0300 - F HCI . ( d ) 0.0500 - F HCI . ( e ) 0.0700 - F HCI . ( f ) 0.0250 - F NH.C1 . * 9 . Calculate ...
... Calculate the pH of a solution prepared by mixing 25.0 ml of 0.0500 - F NH3 with 25.0 ml of ( a ) water . ( b ) 0.0100 - F NaOH . ( c ) 0.0300 - F HCI . ( d ) 0.0500 - F HCI . ( e ) 0.0700 - F HCI . ( f ) 0.0250 - F NH.C1 . * 9 . Calculate ...
Pagina 223
... Calculate the change in pH that occurs when 50.0 ml of 0.0200 - F HCl are added to 50.0 ml of each of the undiluted solutions in Problem 24 . * 27 . Calculate the change in pH that occurs when 50.0 ml of 0.0100 - F NaOH are added to ...
... Calculate the change in pH that occurs when 50.0 ml of 0.0200 - F HCl are added to 50.0 ml of each of the undiluted solutions in Problem 24 . * 27 . Calculate the change in pH that occurs when 50.0 ml of 0.0100 - F NaOH are added to ...
Pagina 311
... Calculate E ° for Ag ( NH3 ) 2 * + e⇒ Ag ( s ) + 2NH3 18. The formation constant for the complex HgCl2 is 1.6 × 1013 . Calculate Eo for the reaction HgCl2 ( aq ) + 2e → Hg ( 1 ) + 2C1 * 19 . Calculate Ksp for Ag2C2O4 given Ag2C2O4 ( s ) ...
... Calculate E ° for Ag ( NH3 ) 2 * + e⇒ Ag ( s ) + 2NH3 18. The formation constant for the complex HgCl2 is 1.6 × 1013 . Calculate Eo for the reaction HgCl2 ( aq ) + 2e → Hg ( 1 ) + 2C1 * 19 . Calculate Ksp for Ag2C2O4 given Ag2C2O4 ( s ) ...
Sommario
Introduction | 1 |
A Review of Simple Equilibrium Constant | 24 |
The Evaluation of Analytical Data | 58 |
Copyright | |
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absorbance absorption acid solution activity coefficient addition AgNO3 aliquot analysis analyte anode application aqueous base buffer cadmium calcium carbonate cathode cation cell cerium(IV chemical color complex concen coulometric determined dilute dissociation constant dissolved EDTA electrode potential electrolyte employed end point Equation equilibrium constant equivalence point equivalent weight error example excess Fe² Fe³ filter flask formal concentration formation formula weight glass gravimetric H₂O H3O+ half-cell half-reaction hydrogen ion hydroxide iodide iodine ionic strength iron(II K₁ liquid measurement membrane mercury(II metal method molar NaOH oxalate oxidation oxidation-reduction particles permanganate polarographic potassium precipitate primary standard quantity radiation react reactants reaction reagent reduced sample saturated silver chloride silver ion silver nitrate sodium solid solubility solution containing species standard electrode potential standard hydrogen electrode standard solution substance sulfuric acid Table temperature thiosulfate titration curves volume volumetric wavelength zinc
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