09:18Ka and acid strength | Chemical processes | MCAT | Khan AcademyKhan Academy Organic Chemistry291
Multiple ChoiceIf the Kb of NH3 is 1.76 x 10-5, determine the acid dissociation constant of its conjugate acid. 74013Has a video solution.
Multiple ChoiceWhich Bronsted-Lowry base has the greatest concentration of hydroxide ions? 4482Has a video solution.
Multiple ChoiceThe Ka value for a weak acid is _________ than the Ka value for a strong acid because the weak acid ionizes to a _________ extent than the strong acid.125
Multiple ChoiceCalculate the pH of a 0.500 M pyridine (C5H5N) solution. Kb value for pyridine is 1.7 × 10−9.390
Multiple ChoiceHypobromous acid (Ka = 2.8 × 10−9) and hydrocyanic acid (Ka = 4.9 × 10−10) are both weak acids. Determine if reactants or products are favored in the following reaction.HBrO (aq) + CN− (aq) ⇌ BrO− (aq) + HCN (aq)a) reactants b) products c) both directions are favored equally d) neither direction is favored20Has a video solution.
Multiple ChoiceIdentify a Bronsted-Lowry acid with weakest conjugate base.a) H3BO3 Ka = 5.4 × 10−10b) HF Ka = 3.5 × 10−4c) HNO2 Ka = 4.6 × 10−4d) HClO Ka = 2.9 × 10−819Has a video solution.
Multiple ChoiceIdentify which of the compounds is the strongest species.a) Iodic acid pKa = 0.80 b) Acetic acid pKb = 9.24 c) Formic acid pKa = 3.75 d) Ammonium pKb = 4.75 18Has a video solution.
Multiple ChoiceDetermine the pKa given the Kb of the following bases:i) NH3 Kb = 1.76 × 10−5 ; NH4+ pKa = ____________ii) C6H5NH2 Kb = 3.9 × 10−10 ; C6H5NH3+ pKa = ____________23Has a video solution.
Textbook QuestionThe following diagrams represent aqueous solutions of three acids, HX, HY, and HZ. The water molecules have been omitted for clarity, and the hydrated proton is represented as H+ rather than H3O+.(b) Which acid would have the smallest aciddissociation constant, Ka? 207Has a video solution.
Textbook QuestionClassify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). d. H2CO3340Has a video solution.
Textbook QuestionThe following pictures represent solutions of three salts NaA (A- = X-, Y-, or Z-); water molecules and Na+ ions have been omitted for clarity. (c) Which A- anion has the smallest value of pKb?88Has a video solution.
Textbook QuestionThe following picture represents the hydrated metal cation M1H2O26 n + , where n = 1, 2, or 3. (a) Write a balanced equation for the reaction of M1H2O26 n + with water and write the equilibrium equation for the reaction.82Has a video solution.
Textbook QuestionThe following picture represents the hydrated metal cation M1H2O26 n + , where n = 1, 2, or 3. (b) Does the equilibrium constant increase, decrease, or remain the same as the value of n increases? Explain.122Has a video solution.
Textbook QuestionRank the solutions in order of decreasing [H3O+]: 0.10 M HCl; 0.10 M HF; 0.10 M HClO; 0.10 M HC6H5O.1521Has a video solution.
Textbook QuestionWrite the chemical equation and the Ka expression for the acid dissociation of each of the following acids in aqueous solution. First show the reaction with H+1aq2 as a product and then with the hydronium ion: (a) C6H5COOH396Has a video solution.
Textbook QuestionChoose from the conjugate acid–base pairs HSO4- >SO42-, HF>F-, and NH4+>NH3 to complete the following equation with the pair that gives an equilibrium constant Kc 7 1. _____ + NO2 - S _____ + HNO2363Has a video solution.
Textbook QuestionThe hypochlorite ion, ClO-, acts as a weak base. (a) Is ClO- a stronger or weaker base than hydroxylamine?1165Has a video solution.
Textbook QuestionWrite the chemical equation and the Kb expression for the reaction of each of the following bases with water: (c) benzoate ion, C6H5CO2-228Has a video solution.
Textbook QuestionWrite the chemical equation and the Kb expression for the reaction of each of the following bases with water: (a) propylamine, C3H7NH2325Has a video solution.
Textbook QuestionUse the acid-dissociation constants in Table 16.3 to arrange these oxyanions from strongest base to weakest: SO42-, CO32-, SO32-, and PO43-.757Has a video solution.
Textbook QuestionWhich is the stronger base, the acetate ion or the hypochlorite ion?274Has a video solution.
Textbook QuestionGiven that Ka for acetic acid is 1.8 * 10-5 and that for hypochlorous acid is 3.0 * 10-8, which is the stronger acid?864Has a video solution.
Textbook QuestionGiven that Kb for ammonia is 1.8 * 10-5 and that for hydroxylamine is 1.1 * 10-8, which is the stronger base?583Has a video solution.
Textbook QuestionPyridinium bromide 1C5H5NHBr2 is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. An aqueous solution of pyridinium bromide has a pH of 2.95. (b) Using Appendix D, calculate the Ka for pyridinium bromide.293Has a video solution.
Textbook QuestionThe Kb for methylamine 1CH3NH22 at 25 °C is given in Appendix D. (a) Write the chemical equation for the equilibrium that corresponds to Kb.299Has a video solution.
Textbook QuestionWrite equations showing how each weak base ionizes water to form OH-. Also write the corresponding expression for Kb. c. C2H5NH2518Has a video solution.
Textbook QuestionWrite equations showing how each weak base ionizes water to form OH-. Also write the corresponding expression for Kb. b. C6H5NH298Has a video solution.
Textbook QuestionWrite equations showing how each weak base ionizes water to form OH-. Also write the corresponding expression for Kb. a. CO32-432Has a video solution.
Textbook QuestionLook up the values of Ka in Appendix C for C6H5OH, HNO3, CH3CO2H, and HOCl, and arrange these acids in order of: (b) Decreasing percent dissociation.235Has a video solution.
Textbook QuestionSalts containing the phosphate ion are added to municipal water supplies to prevent the corrosion of lead pipes. (a) Based on the pKa values for phosphoric acid 1pKa1 = 7.5 * 10 - 3, pKa2 = 6.2 * 10 - 8, pKa3 = 4.2 * 10 - 132 what is the Kb value for the PO43 - ion?165Has a video solution.
Textbook QuestionWhich, if any, of the following statements are true? (a) The stronger the base, the smaller the pKb. (b) The stronger the base, the larger the pKb. (c) The stronger the base, the smaller the Kb. (d) The stronger the base, the larger the Kb. (e) The stronger the base, the smaller the pKa of its conjugate acid. (f) The stronger the base, the larger the pKa of its conjugate acid.9581Has a video solution.
Textbook QuestionButyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84. (a) Calculate the pKb for the butyrate ion.704Has a video solution.
Textbook QuestionWrite a balanced net ionic equation and the corresponding equilibrium equation for the reaction of the following weak bases with water. (c) Cyanide ion, CN119Has a video solution.
Textbook QuestionThe amino acid glycine 1H2N¬CH2¬COOH2 can participate in the following equilibria in water: H2N¬CH2¬COOH + H2OΔ H2N¬CH2¬COO- + H3O+ Ka = 4.3 * 10-3 H2N¬CH2¬COOH + H2OΔ+H3N¬CH2¬COOH + OH- Kb = 6.0 * 10-5 (a) Use the values of Ka and Kb to estimate the equilibrium constant for the intramolecular proton transfer to form a zwitterion: H2N¬CH2¬COOH Δ +H3N¬CH2¬COO-455Has a video solution.
Textbook QuestionUsing values of Kb in Appendix C, calculate values of Ka for each of the following ions. (a) Propylammonium ion, C3H7NH3+404Has a video solution.
Textbook QuestionUsing values of Ka in Appendix C, calculate values of Kb for each of the following ions. (a) Fluoride ion, F-301Has a video solution.
Textbook QuestionNicotine 1C10H14N22 can accept two protons because it has two basic N atoms 1Kb1 = 1.0 * 10-6; Kb2 = 1.3 * 10-112. Calculate the values of Ka for the conjugate acids C10H14N2H+ and C10H14N2H22 + .179Has a video solution.
Textbook QuestionUsing dissociation constants from Appendix D, determine the value for the equilibrium constant for each of the following reactions. (i) HCO3-1aq2 + OH-1aq2 ΔCO32-1aq2 + H2O1l2 (ii) NH4+1aq2 + CO32-1aq2 ΔNH31aq2 + HCO3-1aq2442Has a video solution.
