2. In both instances below, order the acids by increasing pKa a) Al(OH)3 H3ASO, HCIO3 H3PO4 B(OH)3 b) H2S CH4 CH3SH HBr H20 3. Provide the indicate quantity in each case based on Pauling's rules, a) pKa of H2PO4 b) Kb for ClO2 4. Order the hexaqua ions, [M(H2O)6*], of the species below in order of decreasing pKa. Provide a rationale. TI3+ Ca2+ Na* Cd2+

2. In both instances below, order the acids by increasing pKa a) Al(OH)3 H3ASO, HCIO3 H3PO4 B(OH)3 b) H2S CH4 CH3SH HBr H20 3. Provide the indicate quantity in each case based on Pauling's rules, a) pKa of H2PO4 b) Kb for ClO2 4. Order the hexaqua ions, [M(H2O)6], of the species below in order of decreasing pKa. Provide a rationale. TI3+ Ca2+ Na Cd2+

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 136E: Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write...

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1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−
Place the species in each of the following groups in order of increasing acid strength. a. H2O, H2S, H2Se (bond energies: HO, 467 kJ/mol; HS, 363 kJ/mol; HSe, 276 kJ/mol) b. CH3CO2H, FCH2CO2H, F2CHCO2H, F3CCO2H c. NH4+, HONH3+ d. NH4+, PH4+ (bond energies: NH, 391 kJ/mol; PH, 322 kJ/mol) Give reasons for the orders you chose.
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