Analytical ChemistryHolt, Rinehart and Winston, 1979 - 685 pagine |
Dall'interno del libro
Risultati 1-3 di 79
Pagina 81
... Problem 1 . 8. Calculate the absolute and relative standard deviations for the set of data in Problem 2 . * 9 . Compare the absolute and relative standard deviations for the two sets of data in Problem 3 . 10. Compare the absolute and ...
... Problem 1 . 8. Calculate the absolute and relative standard deviations for the set of data in Problem 2 . * 9 . Compare the absolute and relative standard deviations for the two sets of data in Problem 3 . 10. Compare the absolute and ...
Pagina 90
... problem is not possible ; it may , however , be possible to arrive at an approximate solution . 7. Make suitable approximations to simplify the algebra or to decrease the number of unknowns so that the problem can be solved . 8. Solve ...
... problem is not possible ; it may , however , be possible to arrive at an approximate solution . 7. Make suitable approximations to simplify the algebra or to decrease the number of unknowns so that the problem can be solved . 8. Solve ...
Pagina 223
... Problem 23 . 26. 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 ...
... Problem 23 . 26. 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 ...
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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