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AP Chemistry Sample Exam13.What phase change is occuring from point A to point B?(A) Solidification (B) Condensation (C) Sublimation (D) Vaporization (E) Melting14.17. Which represents an acid-base reaction according to theLewis definition but not the Bronsted-Lowry definition?(A) MgCl 2(s) ↔ Mg 2+ (aq) + 2Cl – (aq)(B) CN – (aq) + H 2O(l) ↔ HCN(aq) + OH – (aq)(C) NH 3(g) + HBr(g) ↔ NH 4Br(s)(D) Fe(H 2O) 6 3+ (aq) + H 2O(l) ↔ [Fe(H 2O) 5OH] 2+ (aq) + H 3O + (aq)(E) HF(aq) + OH – (aq) → H 2O(l) + F – (aq)Look at the heating curve for a pure substance above.Which of the following is true about the substance frompoint D to E?(A) Kinetic energy is increasing; potential energy isdecreasing(B) Kinetic energy is decreasing; potential energy isincreasing(C) Kinetic energy is constant; potential energy isdecreasing(D) Kinetic energy is constant; potential energy isincreasing(E) Kinetic energy is increasing; potential energy isconstant18.A water solution of ions is prepared. Based on the Kavalues above, which ions will react with the water toproduce an acid solution at room temperature?15. <strong>The</strong> weight of HNO 3(molecular weight 63.0) in 40.0milliliters of 5.00-molar solution is(A) 5.6 g(D) 12.6 g(B) 8.7 g(E) 13.1 g(C) 10.4 g16. Which of the following is the weakest acid?(A) HClO 3(D) HClO 2(B) HClO 4(E) HClO(C) HClI. Na +II. Fe 3++III. NH 4–IV. HCO 3–V. HSO 4(A) I and II only(B) II and III only(C) I, II, and III only(D) II, III, and V only(E) III, IV, and V onlyPage 2
19. Consider the following:I. PO 43–II. HPO 42–III. H 2PO 4–IV. H 3PO 4<strong>The</strong> term amphiprotic can be used to describe(A) I only(D) II, III and IV only(B) I and II only(E) II and III only(C) I, II and III only20. Which curve best represents the titration of NaOH withHCl?(A)(C)AP Chemistry Sample Exam24. A student mixes 100. mL of 1.00 M calcium hydroxide(aq) with 100. mL of 1.00 M aluminum nitrate (aq).Assuming the hydroxide ion concentration becomesrelatively small, which of the following is true about theincreasing concentration of the remaining ions?(A) [Ca 2+ ] < [NO 3 – ] < [Al 3+ ] (D) [Ca 2+ ] < [Al 3+ ] < [NO 3– ](B) [Al 3+ ] < [NO – 3] < [Ca 2+ ] (E) [Al 3+ ] < [Ca 2+ ] < [NO – 3](C) [NO – 3] < [Al 3+ ] < [Ca 2+ ]25. __CuOH + __O 2+ __H 2O → __Cu(OH) 2If 2 moles of O 2oxidizes CuOH according to theunbalanced equation above, how many moles of Cu(OH) 2can be formed?(A) 2 (D) 6(B) 4 (E) 8(C) 5(B)(D)21. A container is filled with 10.0 L of 0.050 M NaI. What isthe maximum mass of solid Pb(NO 3) 2that can be dissolvedwithout forming a precipitate?(A) 1.1 × 10 –2 g(D) 5.6 × 10 –5 g(B) 2.2 × 10 –3 g(E) 5.6 × 10 –7 g(C) 3.2 × 10 –4 g22. K sp= 7.00 × 10 –9 for BaCO 3K sp= 9.90 × 10 –9 for CaCO 3A 100. mL solution is 0.10 M with respect to Ca(NO 3) 2and0.10 M with respect to Ba(NO 3) 2. If 0.10 M K 2CO 3isadded to the solution in drops until a precipitation occurs,which of the following will occur?(A) Barium carbonate will be the only precipitate.(B) Calcium carbonate will be the only precipitate.(C) Both calcium and barium carbonate will precipitate.(D) Potassium nitrate and barium carbonate willprecipitate.(E) Potassium nitrate and calcium carbonate willprecipitate.23. Mn 2+ + IO 3 – + H 2O → MnO 4 – + ½I 2+ 2H +What is the reducing agent in the reaction above?–(A) IO 3(D) H +(B) H 2O (E) I 2(C) Mn 2+26. As 2O 3+ 2NO 3 – + 2H 2O + 2H + → 2H 3AsO 4+ N 2O 3In this reaction, nitrogen(A) loses electrons and increases in oxidation number(B) gains electrons and increases in oxidation number(C) loses electrons and decreases in oxidation number(D) gains electrons and decreases in oxidation number(E) maintains the number of electrons and the oxidationnumber27. During the electrolysis of a solution of KCl, whatsubstance is produced at the anode?(A) H 2O(l)(D) H 2(g)(B) Cl 2(g)(E) K(s)(C) O 2(g)28. How long would it take, running a current of 9.65 amperes,to deposit 130. g of zinc from a solution of ZnF 2?(A) 4.00 × 10 4 s(D) 4.00 × 10 3 s(B) 2.00 × 10 4 s(E) 2.00 × 10 3 s(C) 1.00 × 10 4 s29.Which species is most readily oxidized?(A) e –(D) Zn(s)(B) Fe 2+ (E) Zn 2+(C) Fe 3+Page 3
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