09:18Ka and acid strength | Chemical processes | MCAT | Khan AcademyKhan Academy Organic Chemistry517views
Multiple ChoiceIf the Kb of NH3 is 1.76 x 10-5, determine the acid dissociation constant of its conjugate acid. 1177views1rank3comments
Multiple ChoiceWhich Bronsted-Lowry base has the greatest concentration of hydroxide ions? 665views2rank
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.388views
Multiple ChoiceCalculate the pH of a 0.500 M pyridine (C5H5N) solution. Kb value for pyridine is 1.7 × 10−9.1143views
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 favored329views4rank
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 × 10−8254views3rank
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 201views
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 = ____________232views3rank
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? 540views
Textbook QuestionClassify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). d. H2CO3588views
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?277views
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.251views
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.312views
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.2663views
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) C6H5COOH897views
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 _____ + HNO2676views
Textbook QuestionThe hypochlorite ion, ClO-, acts as a weak base. (a) Is ClO- a stronger or weaker base than hydroxylamine?2018views
Textbook QuestionWrite the chemical equation and the Kb expression for the reaction of each of the following bases with water: (c) benzoate ion, C6H5CO2-508views
Textbook QuestionWrite the chemical equation and the Kb expression for the reaction of each of the following bases with water: (a) propylamine, C3H7NH2747views
Textbook QuestionUse the acid-dissociation constants in Table 16.3 to arrange these oxyanions from strongest base to weakest: SO42-, CO32-, SO32-, and PO43-.1489views
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?1308views
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?1113views
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.574views
Textbook QuestionThe value of Ka for nitrous acid 1HNO22 at 25 °C is given in Appendix D. (a) Write the chemical equation for the equilibrium that corresponds to Ka.569views
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.607views
Textbook QuestionWrite equations showing how each weak base ionizes water to form OH-. Also write the corresponding expression for Kb. c. C2H5NH2899views
Textbook QuestionWrite equations showing how each weak base ionizes water to form OH-. Also write the corresponding expression for Kb. b. C6H5NH2356views
Textbook QuestionWrite equations showing how each weak base ionizes water to form OH-. Also write the corresponding expression for Kb. a. CO32-949views
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.621views
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?380views
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.1823views1rank
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.1148views
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, CN393views
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-882views
Textbook QuestionUsing values of Kb in Appendix C, calculate values of Ka for each of the following ions. (a) Propylammonium ion, C3H7NH3+823views
Textbook QuestionUsing values of Ka in Appendix C, calculate values of Kb for each of the following ions. (a) Fluoride ion, F-644views
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 + .465views
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 + HCO3-1aq2866views
Open QuestionGiven that Ka for HIO is 3.2×10−11 at 25 °C, what is the value of 𝐾b for IO− at 25 °C?98views
Open QuestionGiven that a base has a Kb value of 8.36×10−4, what is the Ka of its conjugate acid?90views