Analytical Chemistry: An IntroductionHolt, Rinehart and Winston, 1965 - 527 pagine |
Dall'interno del libro
Risultati 1-3 di 85
Pagina 188
... Calculate the milligrams of H2SO4 per milliliter of solution if a 25.0 - ml aliquot required 37.9 ml of 0.0851 N NaOH for complete neutralization . • ans . 6.32 mg per ml 37. What is the percent BaCl2 2H2O if a 0.412 - gram sample ...
... Calculate the milligrams of H2SO4 per milliliter of solution if a 25.0 - ml aliquot required 37.9 ml of 0.0851 N NaOH for complete neutralization . • ans . 6.32 mg per ml 37. What is the percent BaCl2 2H2O if a 0.412 - gram sample ...
Pagina 277
... Calculate the pH of a neutral solution at each of these temperatures . 7.47 at 0 ° C ans . pH = 2. Calculate the [ H3O + ] , [ QH ̄ ] , pH , and pOH of ( a ) 0.200 N HClO , and ( b ) 0.0035 F KOH . ans . ( a ) [ H3O + ] = 0.200 ; [ OH ...
... Calculate the pH of a neutral solution at each of these temperatures . 7.47 at 0 ° C ans . pH = 2. Calculate the [ H3O + ] , [ QH ̄ ] , pH , and pOH of ( a ) 0.200 N HClO , and ( b ) 0.0035 F KOH . ans . ( a ) [ H3O + ] = 0.200 ; [ OH ...
Pagina 343
... Calculate the potentials of the following cells . Indicate which electrode is the anode of a galvanic cell . ( a ) Ag | AgCl ( sat'd ) , KCl ( 1.0 F ) || KCl ( 0.001 F ) , AgCl ( sat'd ) | Ag ( b ) Pt , H2 ( 1 atm ) | HCl ( 0.5 F ...
... Calculate the potentials of the following cells . Indicate which electrode is the anode of a galvanic cell . ( a ) Ag | AgCl ( sat'd ) , KCl ( 1.0 F ) || KCl ( 0.001 F ) , AgCl ( sat'd ) | Ag ( b ) Pt , H2 ( 1 atm ) | HCl ( 0.5 F ...
Sommario
The Scope of Analytical Chemistry | 1 |
Some Elementary Concepts | 7 |
The Evaluation of Analytical Data | 34 |
Copyright | |
21 sezioni non visualizzate
Altre edizioni - Visualizza tutto
Parole e frasi comuni
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