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 × 10−10.207views1rank
Multiple ChoiceAn unknown weak base has an initial concentration of 0.750 M with a pH of 8.03. Calculate its equilibrium base constant. 191views1rank1comments
Textbook QuestionSolve an equilibrium problem (using an ICE table) to calculate the pH of each solution. b. a solution that is 0.16 M in NH3 and 0.22 M in NH4Cl937views
Textbook QuestionSolve an equilibrium problem (using an ICE table) to calculate the pH of each solution. b. 0.15 M NaF504views
Textbook QuestionDetermine the pH of each of the following solutions (Ka and Kb values are given in Appendix D): (c) 0.165 M hydroxylamine.1121views
Textbook QuestionCalculate the pH of 100.0 mL of 0.30 M NH3 before and after the addition of 4.0 g of NH4NO3, and account for the change. Assume that the volume remains constant.581views
Textbook QuestionEphedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic base: C10H15ON1aq2 + H2O1l2 Δ C10H15ONH+1aq2 + OH-1aq2 A 0.035 M solution of ephedrine has a pH of 11.33. (b) Calculate Kb for ephedrine.457views
Textbook QuestionCodeine 1C18H21NO32 is a weak organic base. A 5.0 * 10-3M solution of codeine has a pH of 9.95. Calculate the value of Kb for this substance. What is the pKb for this base?2149views3rank
Textbook QuestionUsing data from Appendix D, calculate 3OH-4 and pH for each of the following solutions: (b) 0.035 M Na2S611views
Textbook QuestionCaffeine (C8H10N4O2) is a weak base with a pKb of 10.4. Calculate the pH of a solution containing a caffeine concentration of 455 mg>L.3265views4rank
Textbook QuestionAmphetamine (C9H13N) is a weak base with a pKb of 4.2. Calculate the pH of a solution containing an amphetamine concentration of 225 mg>L.2423views
Textbook QuestionMorphine is a weak base. A 0.150 M solution of morphine has a pH of 10.7. What is Kb for morphine?3265views1comments
Textbook QuestionCalculate the concentration of all species in a 0.225 M C6H5NH3Cl solution.1627views
Textbook QuestionButyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84. (c) Calculate the pH of a 0.050 M solution of sodium butyrate.1113views
Textbook QuestionStrychnine 1C21H22N2O22, a deadly poison used for killing rodents, is a weak base having Kb = 1.8 * 10-6. Calculate the pH of a saturated solution of strychnine (16 mg/100 mL).544views
Textbook QuestionOxycodone 1C18H21NO42, a narcotic analgesic, is a weak base with pKb = 5.47. Calculate the pH and the concentrations of all species present (C18H21NO4, HC18H21NO4 + , H3O+ , and OH-) in a 0.002 50 M oxycodone solution.735views2comments
Textbook QuestionLactic acid is a weak acid found in milk. Its calcium salt is a source of calcium for growing animals. A saturated solution of this salt, which we can represent as Ca(Lact)2, has a [Ca2 + ] = 0.26 M and a pH = 8.78. Assuming the salt is completely dissociated, calculate the Ka of lactic acid.2885views
Textbook QuestionAcid and base behavior can be observed in solvents other than water. One commonly used solvent is dimethyl sulfoxide (DMSO), which can be treated as a monoprotic acid 'HSol.' Just as water can behave either as an acid or a base, so HSol can behave either as a Brønsted–Lowry acid or base. (b) The weak acid HCN has an acid dissociation constant Ka = 1.3 * 10-13 in the solvent HSol. If 0.010 mol of NaCN is dissolved in 1.00 L of HSol, what is the equilibrium concentration of H2Sol + ?916views
Textbook QuestionIn aqueous solution, sodium acetate behaves as a strong electrolyte, yielding Na+ cations and CH3CO2 - anions. A particular solution of sodium acetate has a pH of 9.07 and a density of 1.0085 g/mL. What is the molality of this solution, and what is its freezing point?1429views
Open QuestionThe Kb of methylamine is 4.4 x 10–4. What is the approximate [OH–] of a 1 M solution of methylamine?87views
Open Questioncalculate the pH of a 0.10 M solution of hydrazine, N2H4 . Kb for hydrazine is 1.3×10−6 .97views
Open QuestionThe pOH of a solution is 10.75. What is the concentration of OH– ions in the solution?94views
Open QuestionDetermine the pH of a 0.227 M C5H5N solution at 25 °C. The Kb of C5H5N is 1.7 x 10-9.84views
Open QuestionThe pH of 2.65 m CH3NH2(aq) is 12.54. determine the value of Kb for methylamine.613views
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?88views
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?99views
Open QuestionDetermine the pH of a 0.227 M C5H5N solution at 25°C. The Kb of C5H5N is 1.7 x 10-9.101views