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 × 10−10.203views1rank
Multiple ChoiceAn unknown weak base has an initial concentration of 0.750 M with a pH of 8.03. Calculate its equilibrium base constant. 190views1rank1comments
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 NH4Cl929views
Textbook QuestionSolve an equilibrium problem (using an ICE table) to calculate the pH of each solution. b. 0.15 M NaF500views
Textbook QuestionDetermine the pH of each of the following solutions (Ka and Kb values are given in Appendix D): (c) 0.165 M hydroxylamine.1112views
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.576views
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.450views
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?2137views3rank
Textbook QuestionUsing data from Appendix D, calculate 3OH-4 and pH for each of the following solutions: (b) 0.035 M Na2S606views
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.3222views4rank
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.2409views
Textbook QuestionMorphine is a weak base. A 0.150 M solution of morphine has a pH of 10.7. What is Kb for morphine?3248views1comments
Textbook QuestionCalculate the concentration of all species in a 0.225 M C6H5NH3Cl solution.1613views
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.1095views
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).537views
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.723views2comments
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.2865views
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 + ?912views
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?1417views
Open QuestionThe Kb of methylamine is 4.4 x 10–4. What is the approximate [OH–] of a 1 M solution of methylamine?86views
Open Questioncalculate the pH of a 0.10 M solution of hydrazine, N2H4 . Kb for hydrazine is 1.3×10−6 .95views
Open QuestionThe pOH of a solution is 10.75. What is the concentration of OH– ions in the solution?90views
Open QuestionDetermine the pH of a 0.227 M C5H5N solution at 25 °C. The Kb of C5H5N is 1.7 x 10-9.83views
Open QuestionThe pH of 2.65 m CH3NH2(aq) is 12.54. determine the value of Kb for methylamine.609views
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?85views
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?95views
Open QuestionDetermine the pH of a 0.227 M C5H5N solution at 25°C. The Kb of C5H5N is 1.7 x 10-9.97views