Multiple ChoiceDetermine the pH of a solution made by dissolving 6.1 g of sodium cyanide, NaCN, in enough water to make a 500.0 mL of solution. (MW of NaCN = 49.01 g/mol). The Ka value of HCN is 4.9 × 10−10.229views3rank
Multiple ChoiceAn unknown weak base has an initial concentration of 0.750 M with a pH of 8.03. Calculate its equilibrium base constant. 208views2rank1comments
Open QuestionThe Kb of methylamine is 4.4 x 10–4. What is the approximate [OH–] of a 1 M solution of methylamine?96views
Open Questioncalculate the pH of a 0.10 M solution of hydrazine, N2H4 . Kb for hydrazine is 1.3×10−6 .110views
Open QuestionThe pOH of a solution is 10.75. What is the concentration of OH– ions in the solution?106views
Open QuestionDetermine the pH of a 0.227 M C5H5N solution at 25 °C. The Kb of C5H5N is 1.7 x 10-9.94views
Open QuestionThe pH of 2.65 m CH3NH2(aq) is 12.54. determine the value of Kb for methylamine.642views
Open QuestionAn unknown weak base with a concentration of 0.170 M has a ph of 9.42. What is the Kb of this base?105views
Open QuestionMorphine is a weak base. a 0.150 m solution of morphine has a pH of 10.5. What is the Kb for morphine?118views
Open QuestionThe pH of 2.65 M CH3NH2(aq) is 12.54. Determine the value of Kb for methylamine.109views
Open QuestionDetermine the pH of a 0.227 M C5H5N solution at 25°C. The Kb of C5H5N is 1.7 x 10-9.126views