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NAME: __________________________ AP CHEMISTRY CHAPTER 11 PROBLEM SET #4 (Questions 1-2) Select the letter that best completes the statement or answers the question. _____ 1. HCN(aq) + H2O(l) -- H3O+(aq) + CN-(aq) In the equilibrium represented above, the species that act as bases include which of the following? I. CN- II. H2O A. B. C. D. E. _____ 2. III. HCN II only III only I and II I and III II and III For oxyacids that vary only by the number of oxygens (i.e., HAO, HAO2, HAO3), which of the following occurs as the number of oxygen atoms increases? A. It is impossible to predict the acid strength. B. The strength of the acid increases. C. The strength of the acid decreases only if A is a nonmetal. D. The strength of the acid decreases only if A is a metal. E. The strength of the acid decreases whether A is a nonmetal or a metal. 3. Arrange the following 0.10 M solutions in order from most acidic to most basic: Ca(NO3)2 NaNO2 HNO3 NH4NO3 Ca(OH)2 4. Calculate the concentrations of all species present in a 0.25 M solution of ethylammonium chloride (C2H5NH3Cl). 5. 6. Calculate the pH of the following solutions: a. 0.12 M NaNO2 b. 0.45 M NaOCl c. 0.40 M NH4ClO4 Consider a solution of an unknown salt having the general formula BHCl, where B is one of the weak bases in the table in your textbook. A 0.10 M solution of the unknown salt has a pH of 5.82. What is the actual formula of the salt. 7. Calculate the pH of a 0.10 M CoCl3 solution. Ka for Co(H2O)63+ is 1.0 X 10-5. 8. Are solutions of the following salts, acidic, basic or neutral? Support your answer. a. KCl 9. b. NH4C2H3O2 c. CH3NH3Cl Place the species in each of the following groups in order of increasing base strength. Give your reasoning for each. a. BrO-, BrO2-, b. ClO2-, BrO2-, BrO3- IO2- 10. Place the species in each of the following groups in order of increasing acid strength. a. H2O, H2S, H2Se (bond energies: H-O, 467 kJ/mol; H-S, 363 kJ/mol; HSe, 276 kJ/mol) b. 11. Will the following oxides give acidic, basic or neutral solutions when dissolved in water? Write reactions to justify your answers. a. Na2O b. 12. CH3CO2H, FCH2CO2H, F2CHCO2H, F3CCO2H P4O10 Identify the Lewis acid and the Lewis base in each of the following reactions: a. I2 + I- b. Zn(OH)2 + 2OH- ----- ----- I3- Zn(OH)42- c. 13. Fe3+ + SCN- - FeSCN2+ Calculate the pH of a 10.0 mL solution of C18H21NO3 containing 5.0 mg of C18H21NO3 if the pKb is 6.05. (pKb = -log Kb). This is a solution that produces a base. ANSWERS: 1. C 2. B 3. HNO3, NH4NO3, Ca(NO3), NaNO2, Ca(OH)2 4. [H+] and [C2H5NH2] = 2.1 X 10-6 M [C2H5NH3+] = .25 M (.25 – 2.1X 10-6 = .25 with sig figs) [OH-] = 4.8 X 10-9 M 5. a. 8.23 b. 10.56 c. 4.82 6. CH3NH2- methylamine 7. 3.00 8. a. neutral b. neutral c. acidic 9. a. BrO3- < BrO2- < BrOb. HClO2- < HBrO2 < HIO210. a. H2O < H2S < H2Se b. CH3CO2H, FCH2CO2H, F2CHCO2H, F3CCO2H 11. a. basic b. acidic 12. a. I2 = acid; I- = basic b. Zn(OH)2 = acid; OH- = base c. Fe3+ = acid; SCN- = base 13. 9.59