<p> Chemistry 116: General Chemistry Syracuse University Project Advance Exam #2, Spring 2005</p><p>Name Date </p><p>-7 -11 (1) Carbonic acid is a diprotic acid, H2CO3, with Ka1 = 4.2 x 10 and Ka2 = 4.8 x 10 . The ion -14 product for water is Kw = 1.0 x 10 .</p><p>What is the equilibrium constant for the following carbonic acid reaction?</p><p>+ 2- H2CO3 + 2H2O 2H3O + CO3</p><p>(a) 2.1 x 10-4 (b) 2.0 x 10-17 (c) 4.2 x 10-7 (d) 4.8 x 10-11 (e) 2.4 x 10-8</p><p>(2) Label in order, left to right, the Bronsted Lowrey acids and bases in the following reaction:</p><p>- 2- + NH3 + HSO4 SO4 + NH4</p><p>(a) acid, base, base, acid (b) base, acid, base, acid (c) base, acid, acid, base (d) acid, base, acid, base (e) none of the above</p><p>+ (3) What is the concentration of H3O in a solution of 0.075M KOH at 25°C?</p><p>(a) 0.075M (b) 0.150M (c) 1.33 x 10-13M (d) 6.66 x 10-14M (e) none of the above</p><p>- (4) What is the concentration of OH in a 1.0M solution of aniline, C6H5NH2? -10 (Kb = 4.2 x 10 )</p><p>(a) 2.0 x 10-5M (b) 2.0 x 10-6 (c) 4.2 x 10-5M (d) 4.2 x 10-6 M (e) none of the above</p><p>(5) What is the minimum concentration of Mg2+ that is needed to begin the formation of a precipitate of Mg(OH)2 in an aqueous solution of pH = 10.0? </p><p>CHE 116 1 Spring 2005 Exam #2 -12 (Ksp of Mg(OH)2 equals 6 x 10 ).</p><p>(a) 3 x 10-8M (b) 3 x 10-4 (c) 1.5 x 10-4M (d) 6 x 10-8M (e) 6 x 10-4M</p><p>(6) Which of the following is a weak electrolyte in aqueous solution?</p><p>(a) H2SO4 (b) KOH (c) NH3 (d) NaClO4 (e) HI</p><p>(7) A saturated solution of PbBr2 is prepared by dissolving the solid salt in water. The 2+ concentration of Pb in solution is found to be 0.0115 M. The Ksp for PbBr2 is</p><p>(a) 4.9 x 10-5 (b) 2.3 x 10-2 (c) 1.2 x 10-5 (d) 6.1 x 10-6 (e) 2.6 x 10-4</p><p>(8) A 0.010 M aqueous solution of a weak acid HX has a pH of 4.00. What is the percentage dissociation of HX in the solution?</p><p>(a) 0.010% (b) 10% (c) 0.10% (d) 0.0010% (e) 1.0%</p><p>(9) The solubility of PbSO4 is 0.041 g/L. Its molar mass is 303 g/mol. Its Ksp is</p><p>(a) 1.3 x 10-4 (b) 8.8 x 10-12 (c) 1.7 x 10-3 (d) 4.1 x 10-2 (e) 1.7 x 10-8</p><p>(10) Which of the following statements is/are correct?</p><p>1. The pH of a vinegar (acetic acid) solution at 25°C is greater than 7.0. CHE 116 2 Spring 2005 Exam #2 2. The hydroxide ion concentration of a 0.35M solution of Ba(OH)2 is 0.70M. 3. The hydroxide ion concentration of a 2.5M solution of HCl at 25°C is 4.0 x 10-15M.</p><p>(a) 1 (b) 2 (c) 1 and 2 (d) 1 and 3 (e) 2 and 3</p><p>(11) Which of the following statements is/are correct?</p><p>1. In the following reaction, CN- acts as a Lewis base: 3+ - 3- Fe + 6CN  [Fe(CN)6]</p><p>2. In the following proton-transfer reaction, Bronsted-Lowrey acids and bases are correctly labeled: 2- + - HPO4 + NH4 H2PO4 + NH3 acid base acid base - + 3. In the following reaction, HSO3 and NH4 are a Bronsted-Lowrey conjugate acid-base 2- + - pair: SO3 and NH4 HSO3 + NH3</p><p>(a) 1 (b) 2 (c) 3 (d) 1 and 2 (e) 2 and 3</p><p>+ (12) What is the concentration of the conjugate acid, C6H5NH3 , in a 1.0M aqueous solution of the -10 weak base aniline, C6H5NH2? Kb = 4.2 x 10</p><p>(a) 4.2 x 10-5M (b) 2.0 x 10-5M (c) 2.0 x 10-10M (d) 4.2 x 10-10M (e) none of the above</p><p>(13) Which of the following statements is/are correct?</p><p>1. An aqueous solution of BaClO4 is basic. 2. An aqueous solution of NH4I is acidic. 3. An aqueous solution of KC2H3O2 (potassium acetate) is acidic.</p><p>(a) 1 (b) 2 (c) 3 (d) 1 and 2 (e) 2 and 3 (14) The solubility product constant for Iron(III) hydroxide, Fe(OH)3, in pure water at 25°C is Ksp -39 = 2.5 x 10 . Calculate the molar solubility of Fe(OH)3 in pure water (Set-up only).</p><p>CHE 116 3 Spring 2005 Exam #2 2 . 5 x 1 0 3 9 (a) 2 2 7</p><p>2 . 5 x 1 0 3 9 (b) 3  2 7</p><p>2 . 5 x 1 0 3 9 (c) 4  2 7</p><p>(c) 2 2.5x10 39  (e) 4 2.5x10 39 </p><p>+ - (15) H2SO3(aq) + H2O(l) H3O (aq) + HSO3 (aq)  - + 2- HSO3 (aq) + H2O(l) H3O (aq) + SO3 (aq)</p><p>In the above reversible reactions, which are the Bronsted acids?</p><p>- 2- (a) HSO3 , H2O, SO3 + - (b) H2O, H3O , HSO3 - (c) H2SO3, H2O, HSO3 + -2 (d) H3O , H2O, SO3 + - (e) H2SO3, H3O , HSO3</p><p>(16) Calculate the pH of a 0.017 M Ba(OH)2 solution.</p><p>(a) 12.13 (b) 0.034 (c) 1.77 (d) 12.53 (e) 1.47</p><p>(17) The ionization constant of water at 45°C is 4.0 x 10-14. What is the pH of pure water at this temperature?</p><p>+ - H2O H (aq) + OH (aq)</p><p>(a) 7.00 (b) 6.70 (c) 13.40 (d) 5.70 (e) 7.70</p><p>(18) The pH of a 0.10 M NH4Cl solution is 5.13. The hydroxide-ion concentration of this solution is</p><p>(a) 1.0 x 10-13 M (b) 1.3 x 10-9 M CHE 116 4 Spring 2005 Exam #2 (c) 7.4 x 10-6 M (d) 1.3 x 10-5 M (e) none of these.</p><p>(19) A solution that is formed by combining 700 mL of 0.20 M HCl with 300 mL of 0.50 M NaOH + has an H3O concentration of</p><p>(a) 1 x 10-12 (b) 0.2 (c) 0.01 (d) 0.02 (e) 0.14</p><p>(20) Calculate the pH of a solution prepared by dissolving 0.37 moles of formic acid (HCO2H) and -4 0.23 moles of sodium formate (NaCO2H) in 1.00 L of solution. (Ka = 1.8 x 10 )</p><p>(a) 2.09 (b) 10.46 (c) 3.54 (d) 2.30 (e) none of the above</p><p>-4 (21) Determine the pH of a 0.15 M solution of KF. Ka = 7.0 x 10 ).</p><p>(a) 12.01 (b) 5.83 (c) 8.17 (d) 2.33 (e) 3.46</p><p>(22) Which one of the following has the lowest ionization energy? A) iodine B) bromine C) chlorine D) fluorine E) oxygen</p><p>(23) In the Periodic Table of the Elements, all the elements in Group 16 have the same number of</p><p>(a) valence electrons (b) energy levels (c) protons (d) neutrons (e) orbitals</p><p>(24) Nonmetals in the solid state are poor conductors of heat and tend to </p><p>(a) be brittle (b) be malleable (c) have luster (d) have good electrical conductivity CHE 116 5 Spring 2005 Exam #2 (f) all of the above</p><p>(25) Which element in Group 15 has the most metallic character?</p><p>(a) N (b) P (c) As (d) Bi</p><p>CHE 116 6 Spring 2005 Exam #2</p>