AP Chemistry Campbell

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Bathsheba Ball
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1 11. The molar mass of magnesium carbonate is (A) 80.0 g mol 1 (B) 84.3 g mol 1 (C) 88.2 g mol 1 (D) 82.0 g mol When the equation below is written and balanced, what is the coefficient for the hydrochloric acid? Sodium reacts with hydrochloric acid to yield sodium chloride and hydrogen gas. (A) 1 (B) 2 (C) 3 (D) Which of the following is always true when a chemical equation is fully balanced? (A) The sum of the coefficients of reactants equals the sum of the coefficients of the products. (B) The volume of the reactants will equal the volume of the products. (C) The energy stored in the reactant chemical bonds will equal the energy stored in the products chemical bonds. (D) The mass of the reactants will equal the mass of the products. 14. The concept of the mole is based on having the same number of particles as there is found in 12.0 g of which element? (A) Hydrogen (B) Helium (C) Carbon (D) Neon 15. Boron obtained from borax deposits in Death Valley consists of two isotopes. They are boron-10 and boron-11 with atomic masses of amu and amu, respectively. The atomic mass of boron is amu (see periodic table). Which isotope of boron is more abundant, boron-10 or boron-11? A) Cannot be determined from data given B) Neither, their abundances are the same. C) Boron-10 D) Boron The element oxygen consists of three naturally occurring isotopes: 16O, 17O, and 18O. The atomic mass of oxygen is 16.0 amu. What can be implied about the relative abundances of these isotopes? A) More than 50% of all O atoms are 17O. B) Almost all O atoms are 18O. C) Almost all O atoms are 17O. D) The isotopes all have the same abundance, i.e. 33.3%. E) The abundances of 17O and 18O are very small.

2 17. What is the average mass of one Ca atom? A) amu D) 2.41 x amu B) g E) 2.41x10 25 g C) g/mol 18. Which of the following NH3 samples contains the greatest number of moles of NH3? A) moles NH3 D) 8.90g NH3 B) 4.65 x NH3 molecules E) 6.78 x 10 1 g NH3 C) 6.78 x NH3 molecules 19. A mass spectrometer works by ionizing atoms or molecules, and then accelerating them through oppositely charged plates. The mass is obtained by A) Measuring the force of impact on a detecting screen, and then calculating the mass using force = mass acceleration. B) Suspending the ions in an applied electric field, and then calculating mass by the setting the downward gravitational force equal to the upward electrostatic force. C) Measuring the magnitude of deflection as the ions pass through a magnetic field to obtain the charge-to-mass ratio, and then calculating the mass from that ratio. D) Measuring the time it takes for the ions to hit the detector at a known distance to calculate the acceleration, and then calculating mass from force = mass acceleration. 20. Which of the following compounds is a strong electrolyte? A) H2O B) CH3OH C) CH3CH2OH D) HF E) NaF 21. Which of the following compounds is a weak electrolyte? A) HNO3 B) NaNO3 C) HNO2 D) NaNO2 E) NaOH 22. Which of the following compounds is a nonelectrolyte? A) NaF B) HNO3 C) CH3COOH (acetic acid) D) NaOH E) C6H12O6 (glucose)

3 23. The distinguishing characteristic of all electrolyte solutions is that they: A) Contain molecules. D) Always contain acids. B) Conduct electricity. E) Conduct heat. C) React with other solutions. 24. Based on the solubility rules, which one of the following compounds should be insoluble in water? A) NaCl B) MgBr2 C) FeCl2 D) AgBr E) ZnCl2 25. Which of the following will occur when a solution of Pb(NO3)2(aq) is mixed with a solution of KI(aq)? A) A precipitate of KNO3 will form; Pb 2+ and I are spectator ions. B) No precipitate will form. C) A precipitate of Pb(NO3)2 will form; K + and I are spectator ions. D) A precipitate of PbI2 will form; K + and NO3 are spectator ions. E) A precipitate of PbI2 will form; Pb 2+ and I are spectator ions. 26. The common constituent in all acid solutions is A) H2 B) H + C) OH D) H2SO4 E) Cl 27. Which of the following compounds is a weak acid? A) HF B) HCl C) HBr D) HI E) HClO4 28. Which of the following compounds is a strong acid? A) HF B) HI C) HClO2 D) H2SO3 E) HNO2 29. Which of the following compounds is a weak base? A) KOH B) Sc(OH)3 C) NH3 D) NH4 + E) CO2 30. Identify the correct net ionic equation for the reaction that occurs when solutions of HF and KOH are mixed. A) H + (aq) + OH - (aq) H2O(l) B) HF(aq) + OH - (aq) H2O(l) + F - (aq) C) H + (aq) + KOH(aq) H2O(l) + K + (aq) D) HF(aq) + KOH(aq) H2O(l) + KF(s) E) HF(aq) + KOH(s) H2O(l) + KF(aq) 31. The oxidation number of Mn in KMnO4 is A) +8 B) +7 C) +5 D) 7 E) The oxidation number of Fe in K3Fe(CN)6 is A) +3 B) +2 C) +1 D) 3 E) 4

4 33. For the chlorate ion, ClO3 -, what are the oxidation states of the Cl and O, respectively? A) 1, 2 B) +5, 2 C) +6, 2 D) +7, 2 E) +2, For which one of the following acids is chlorine in the +5 oxidation state? A) HCl B) HClO C) HClO2 D) HClO3 E) HClO4 35. Determine the correct oxidation numbers for all three elements in Rb2SO3 in the order that the elements are shown in the formula. A) 2, +6, 2 B) 1, +4, 3 C) +2, +4, 2 D) +1, +4, 2 E) +1, +6, Using the redox reaction below determine which element is oxidized and which is reduced. 4NH3 + 3Ca(ClO)2 2N2 + 6H2O + 3CaCl2 A) H is oxidized and N is reduced D) Cl is oxidized and O is reduced B) N is oxidized and Cl is reduced E) Cl is oxidized and N is reduced C) N is oxidized and O is reduced 37. How many total electrons are transferred in the following reaction? B2H6(g) + 3O2(g) B2O3(s) + 3H2O(l) A) 2 B) 3 C) 4 D) 6 E) Which one of the following is a redox reaction? A) 2Al(s) + 3H2SO4(aq) Al2(SO4)3(aq) + 3H2(g) B) 2KBr(aq) + Pb(NO3)2(aq) 2KNO3(aq) + PbBr2(s) C) CaBr2(aq) + H2SO4(aq) CaSO4(s) + 2HBr(g) D) H + (aq) + OH (aq) H2O(l) E) CO3 2 (aq) + HSO4 (aq) HCO3 (aq) + SO4 2 (aq) 39. Identify the reducing agent in the following chemical reaction. 5Fe 2+ (aq) + MnO4 (aq) + 8H + (aq) 5Fe 3+ (aq) + Mn 2+ (aq) + 4H2O (l) A) Fe 2+ B) MnO4 C) H + D) Mn 2+ E) Fe Predict the products of the following single replacement reaction. Fe(s) + CuSO4(aq) A) Cu(s) + FeSO4(aq) D) FeCuSO4(aq) B) Fe(s) + Cu(s) + SO4(aq) E) FeO(s) + CuSO3(aq) C) CuS(s) + Fe2SO4(aq)

5 41. Which of the following is an example of a disproportionation reaction? B) 2KBr(aq) + Cl2(g) 2KCl(aq) + Br2(l) C) 2H2O2(aq) 2H2O(l) + O2(g) D) CaBr2(aq) + H2SO4(aq) CaSO4(s) + 2HBr(g) 42. Which of the following represents a precipitation reaction? A) 2H2(g) + O2(g) 2H2O(l) B) CaBr2(aq) + H2SO4(aq) CaSO4(s) + 2HBr(g) C) 2KNO3(s) 2KNO2(s) + O2(g) D) 2KBr(aq) + Cl2(g) 2KCl(aq) + Br2(l) 43. Which of the following represents a hydrogen displacement reaction? B) 2KBr(aq) + Cl2(g) 2KCl(aq) + Br2(l) C) N2(g) + 3H2(g) 2NH3(g) D) CaBr2(aq) + H2SO4(aq) CaSO4(s) + 2HBr(g) 44. Which of the following represents a combustion reaction? B) LiOH(aq) + HNO3(aq) LiNO3(aq) + H2O(l) C) N2(g) + 3H2(g) 2NH3(g) D) 2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g) 45. Which substance is acting as a Brønsted acid in the following reaction? A) NH4 + B) HSO4 C) H2SO4 D) NH3 HSO4 + NH4 + H2SO4 + NH3 46. Identify the conjugate acid in the following reaction. NH3 + H2O NH4 + + OH A) NH3 B) H2O C) NH4 + D) OH

Aqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined).

Aqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined). Aqueous Reactions Defining Aqueous Reactions Aqueous reactions are reactions that take place in water. To understand them, it is important to understand how compounds behave in water. Some compounds are