Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 86
Pagina 201
... Preparation of Buffers . In principle a buffer solution of any desired pH can be prepared by combining calculated quantities of a suitable conjugate acid - base pair . In practice , however , buffers prepared in this way are found to ...
... Preparation of Buffers . In principle a buffer solution of any desired pH can be prepared by combining calculated quantities of a suitable conjugate acid - base pair . In practice , however , buffers prepared in this way are found to ...
Pagina 221
... prepared by mixing 25.0 ml of 0.0300 - F NaOH with 25.0 ml of ( a ) water . ( b ) 0.0200 - F Ba ( OH ) 2 . ( c ) 0.0300 - F HCI . ( d ) 0.0200 - F HCI . ( e ) 0.0400 - F HCl . ( f ) 0.0200 - F NH3 . * 7 . Calculate the pH of a solution ...
... prepared by mixing 25.0 ml of 0.0300 - F NaOH with 25.0 ml of ( a ) water . ( b ) 0.0200 - F Ba ( OH ) 2 . ( c ) 0.0300 - F HCI . ( d ) 0.0200 - F HCI . ( e ) 0.0400 - F HCl . ( f ) 0.0200 - F NH3 . * 7 . Calculate the pH of a solution ...
Pagina 228
... prepared by diluting an approximate volume of the concentrated reagent and standardizing it against a primary standard base . Less frequently the composition of the concentrated acid is established through careful density measurement ...
... prepared by diluting an approximate volume of the concentrated reagent and standardizing it against a primary standard base . Less frequently the composition of the concentrated acid is established through careful density measurement ...
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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