Chem 401 Unit 2 Exam Spr 2018 (Acids/ Bases/ General Equilibria /Acid-Base Equilibria)

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1 Name: Date: Exam #: _ Chem 401 Unit 2 Exam Spr 2018 (Acids/ Bases/ General Equilibria /Acid-Base Equilibria) Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. (2.5 pts each) 1. For a chemical system at equilibrium, a. the concentrations of reactants and products are equal. b. the partial pressures of reactants and products are equal. c. the forward and reverse reaction rates are equal. d. the rate constants for the forward and reverse reactions are equal. e. the concentrations of the products divided by reactants equals one. 2. Assume that the following endothermic chemical reaction is at equilibrium. C(s) + H 2 O(g) H 2 (g) + CO(g) All of the following will shift the position of the equilibrium to the right EXCEPT a. increasing the temperature. b. increasing the volume. c. decreasing the pressure d. addition of solid carbon. e. removal of a gaseous product. 3. A 2.00 L flask is filled with 2.5 mol SO 3, 2.0 mol SO 2, and 0.40 mol O 2, and allowed to reach equilibrium. Predict the effect on the concentrations of SO 3 as equilibrium is achieved by using Q, the reaction quotient. Assume the temperature of mixture is chosen so that K c = SO 3 (g) 2 SO 2 (g) + O 2 (g) a. [SO 3 ] will decrease because Q < K. b. [SO 3 ] will decrease because Q > K. c. [SO 3 ] will increase because Q < K. d. [SO 3 ] will increase because Q > K. e. [SO 3 ] will remain the same because Q = K. 4. In which of the following equilibrium systems would a decrease in volume have no effect on the concentrations of products and reactants? a. CaCO 3 (s) CaO(s) + CO 2 (g) b. N 2 (g) + 3 H 2 (g) 2 NH 3 (g) c. H 2 (g) + CO 2 (g) CO(g) + H 2 O(g) d. 3 O 2 (g) 2 O 3 (g) e. 2 H 2 O 2 (g) 2 H 2 O(g) + O 2 (g) 5. Which of the following is NOT a strong base? a. Ba(OH) 2 b. Mg(OH) 2 c. LiOH d. CsOH e. All of the above are strong bases. 1

2 Name: 6. Given the following chemical equilibria, N 2 (g) + 2 O 2 (g) 2 NO 2 (g) K 1 N 2 (g) + 2 O 2 (g) N 2 O 4 (g) K 2 Determine the equilibrium constant for the dimerization of nitrogen dioxide. 2 NO 2 (g) N 2 O 4 (g) K 3 a. K 3 = K 1 + K 2 c. K 3 = K 1 K 2 e. K 3 = K 2 b. K 3 = K 1 - K 2 d. K 3 = K 1 K 2 K 1 7. According to the Brønsted-Lowry definition, an acid a. increases the H 3 O + concentration in a solution. b. increases the OH - concentration in a solution. c. is a proton donor. d. is a proton acceptor. e. has a lone pair of electrons that can bond to a proton. 8. Acids that ionize extensively in solution are referred to as a. strong acids. d. Brønsted-Lowry acids. b. weak acids. e. amphiprotic. c. Arrhenius acids. 9. For the reaction below the equilibrium constant, K p, is 1.32 at 627ºC. What is the equilibrium constant, Kc, for the reaction? a b c d e SO 3 (g) SO 2 (g) + 1/2 O 2 (g) 10. Kc = and H = kj/mol at 25 C for the reaction 2 SO 2 (g) + O 2 (g) 2 SO 3 (g). Calculate the value of Kc at 42 C. a b c d e. none of the above 2

3 Name: 11. We place mol N 2 O 4 (g) in a 4.00 L flask at 200 C. After reaching equilibrium, the concentration of NO 2 (g) is M. What is K c for the reaction below at 200 C? N 2 O 4 (g) 2 NO 2 (g) a b c d e All of the following ions are amphiprotic EXCEPT a. HPO 2-4 d. HS - b. H 2 PO - 4 e. CH 3 CO - 2 c. HCO Of the following salts, which one forms a 0.1 M solution with the highest ph? a. KCl b. NH 4 Cl c. KNO 2 d. Ca(NO 3 ) Of the following list of molecules and ions, which are Lewis acids: NH 3, Cl -, Al 3+, BH 3? a. NH 3 only b. Al 3+ only c. NH 3 and Cl - d. Al 3+ and BH 3 e. Cl - and BH Which of the following chemical reactions corresponds to the acid ionization constant, K a, for hydrogen carbonate ion (HCO 3- )? a. HCO 3- (aq) + OH - (aq) CO 2-3 (aq) + H 2 O( ) b. HCO 3- (aq) + H 3 O + (aq) H 2 CO 3 (aq) + H 2 O( ) c. HCO 3- (aq) + H 3 O + (aq) CO 2 (g) + 2 H 2 O( ) d. HCO 3- (aq) CO 2 (g) + OH - (aq) e. HCO 3- (aq) + H 2 O( ) CO 2-3 (aq) + H 3 O + (aq) 16. Which of the following will have the strongest conjugate base? a. acetic acid, K a = b. benzoic acid, K a = c. dihydrogen phosphate ion, K a = d. formic acid, K a = e. hydrocyanic acid, K a =

4 Name: 17. What is the ph of M Sr(OH) 2 at 25ºC? a b c d e Calculate the hydronium ion concentration in an aqueous solution with a poh of 9.85 at 25 C. a M b M c M d M e M 19. In a triprotic acid, which K a has the largest value? a. K a1 b. K a2 c. K a3 d. It depends on the acid 20. Place the following in order of increasing acid strength. HBrO 2 HBrO 3 HBrO HBrO 4 a. HBrO 2 < HBrO 4 < HBrO < HBrO 3 b. HBrO < HBrO 2 < HBrO 3 < HBrO 4 c. HBrO 2 < HBrO 3 < HBrO 4 < HBrO d. HBrO 4 < HBrO 2 < HBrO 3 < HBrO e. HBrO < HBrO 4 < HBrO 3 < HBrO Calculate Gº for the following reaction at 298 K, N 2 O 4 (g) 2 NO 2 (g) given K = a kj b kj c kj d kj e kj 22. Which of the following is an Arrhenius base? a. CH 3 CO 2 H b. RbOH c. CH 3 OH d. KBr e. More than one of these compounds is an Arrhenius base. 4

5 Name: 23. Benzoic acid has a pk a value of What is the value of K b for sodium benzoate? a b c d e Calculate P [NO] eq, if P [NOCl] eq = 0.33 atm, P [Cl 2 ] eq = 0.50 atm, and K p = NOCl(g) 2 NO(g) + Cl 2 (g) a. 1.7 atm b atm c atm d atm e atm Short Answer 25. Write the formula for the a) conjugate acid of NH - 2 _ (2 pts) b) conjugate base of HCO - 3 _ (2 pts) c) the strongest base that can exist in water (2 pts) 26. An acid that can donate more than one hydrogen ion into solution is a acid (2 pts) 27. Write the equillibrium constant expression for Kc for the reaction: (3 pts) Fe 2 O 3 (s) + 3 CO(g) 2 Fe(l) + 3 CO 2 (g) Kc =. 5

6 Name: 28. Write the total, ionic, and net ionic equations for the reaction of a solution of sodium hydroxide with a solution of iron (III) nitrate. (6 pts) SHOW YOUR WORK! Include all charges and state symbols. Problem 29. At a certain temperature, Kp = 1.42 for the reaction PCl 5 (g) PCl 3 (g) + Cl 2 (g). Calculate the equilibrium partial pressures if the initial partial pressures are PCl 5 (g)=3.00atm, PCl 3 (g)=2.00atm, and Cl 2 (g)=2.50atm. (7 pts). 6

7 Name: 30. The ph of M solution of a weak base is What is the value of K b for this base? (4 pts). 31. What is the ph of a 0.75 M solution of sodium cyanide, NaCN? (K a for HCN= ) (6 pts). 7

8 Name: 32. A weak acid HA has a Ka = 4.5 x Calculate the ph and % dissociation in a 0.10M solution of this acid. (6pts). Case 33. Extra Credit: (5 pts) How many kg of limestone (CaCO 3 ) is required to completely neutralize a 4.8 billion liter lake with a ph of 5.40? 8

9 Periodic Table of the Elements A 8A 1 H A 13 3A 14 4A 15 5A 16 6A 17 7A 2 He Li Be B C N O F Ne Na Mg B 4 4B 5 5B 6 6B 7 7B 8 8B 9 8B 10 8B 11 1B 12 2B 13 Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo (98) 44 Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba * 71 Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po (209) 85 At (210) 86 Rn (222) 87 Fr (223) 88 Ra ** 103 (262) 104 (261) 105 (262) 106 (266) 107 (264) 108 (269) 109 (268) 110 (271) 111 (272) 112 (285) 113 (284) 114 (289) 115 (288) 116 (292) 117 (293) 118 (294) *Lanthanides 57 La Ce Pr Nd (145) 62 Sm Eu Gd Tb Dy Ho Er Tm Yb **Actinides 89 Ac Th Pa U (244) 95 (243) 96 (247) 97 (247) 98 (251) 99 (252) 100 (257) 101 (258) 102 (259)

10 SOLUBILITY RULES A SUMMARY OF SOLUBILITIES RULE EXCEPTIONS 1. Nitrates and acetates are generally No common ones. Silver acetate, mercurous acetate, soluble. and lead acetate are moderately soluble. 2. compounds of the alkali metals and the No common ones. ammonium ion are generally soluble. 3. Chlorides, bromides, and iodides are The halides of Ag 1+, Hg 2+ 2, and Pb 2+ ; also HgI 2, BiOCl, generally soluble. and SbOCl. 4. Sulfates are generally soluble. PbSO 4, SrSO 4, and BaSO 4 are insoluble. CaSO 4, Hg 2SO 4, and Ag 2SO 4 are moderately soluble. The corresponding bisulfates are more soluble. 5. Carbonates, chromates, phosphates, and sulfites are generally insoluble. Those of the alkali metals and ammonium ion are soluble. Many acid phosphates are soluble, i.e., Mg(H 2PO 4) 2 and Ca(H 2PO 4) Sulfides are generally insoluble. Those of the alkali metals and ammonium ion are soluble. The alkaline earth metals are soluble. Cr 2S 3 and Al 2S 3 decompose and precipitate as hydroxides. 7. Hydroxides are generally insoluble. Those of the alkali metals and ammonium ion are soluble. The hydroxides of Ba, Sr, and Ca are moderately soluble, i.e., Ca(OH) C = 0.02M (Consider theses strong electrolytes in water.) The hydroxide of Mg is only very lightly soluble, i.e. Mg(OH) C = M (Consider this an insoluble substance.) 8. Almost all ionic compounds containing NO2 -, ClO4 -, ClO3 -, ClO2 -, and ClO - are soluble. 9. All inorganic acids are soluble. Solubility of organic acids is variable. SOLUTIONS MADE FROM THE ABOVE SPECIES, WHEN SOLUBLE, ARE FOUND TO EXIST AS CHARGED PARTICLES AND THUS CONDUCT ELECTRIC CURRENT.

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