Unit 6 Study Guide 6. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? Al + Fe3O4 Al2O3 + Fe A) 1 B) 3 C) 6 D) 9 E) 12 1. All of the following are clues that a chemical reaction has taken place except A) A color change occurs. B) A solid forms. C) The reactant is smaller. D) Bubbles form. E) A flame occurs. 2. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? Sn + NaOH Na2SnO2 + H2 A) 1 B) 2 C) 3 D) 4 E) 5 7. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? CH3OH + O2 CO2 + H2O A) 1 B) 2 C) 3 D) 4 E) 6 3. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? Na2S2O3 + I2 NaI + Na2S4O6 A) 1 B) 2 C) 3 D) 4 E) 6 8. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? P4O10 + H2O H3PO4 A) 10 B) 6 C) 4 D) 2 E) 1 4. You are asked to balance the chemical equation H2 + O2 H2O. How many of the following ways are correct ways to balance this equation? I. 2H2 + O2 2H2O II. H2 + 1 2 O2 H2O III. 4H2 + 2O2 4H2O IV. H2 + O2 H2O2 A) 0 B) 1 C) 2 D) 3 E) 4 9. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? NO2 + H2O HNO3 + NO A) 1 B) 2 C) 3 D) 4 E) 5 10. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? MnO2 + HCl MnCl2 + Cl2 + H2O A) 5 B) 4 C) 3 D) 2 E) 1 5. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? Pb(NO3)2 + K2CO3 PbCO3 + KNO3 A) 5 B) 4 C) 3 D) 2 E) 1 Page 1 16. Consider a reaction given by the equation aA + bB cC + dD. In this equation A, B, C, D represent chemicals, and a, b, c, d represent coefficients in the balanced equation. For a given reaction, how many values are there for the quantity “c/d”? A) 1 B) 2 C) 3 D) 4 E) an infinite number 11. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? PCl5 + H2O H3PO4 + HCl A) 1 B) 2 C) 3 D) 4 E) 5 Use the following to answer questions 17-23: 12. Balance the following equation in standard form and determine the sum of the coefficients. LiAlH4(s) + AlCl3(s) AlH3(s) + LiCl(s) A) 8 B) 9 C) 10 D) 11 E) 12 When the following equations are balanced using the smallest possible integers, what is the number in front of the underlined substance in each case? 13. Which of the following statments is not true of balancing a chemical equation? A) Subscripts in the reactants must be conserved in the products. B) Coefficients are used to balance the atoms on both sides. C) The law of conservation of matter must be followed. D) Phases are often shown for each compound but are not critical to balancing an equation. E) All of the above statements (a-d) are true. 17. Pb(s) + AgNO3(aq) Pb(NO3)2 + Ag(s) A) 1 B) 2 C) 4 D) 5 E) 6 18. S(s) + O2(g) SO2(g) A) 1 B) 2 C) 3 D) 4 E) 5 19. N2(g) + O2(g) N2O3 A) 1 B) 2 C) 3 D) 4 E) 6 20. Al2O3(s) + H2SO4(aq) Al2(SO4)3(aq) + H2O(l) A) 1 B) 2 C) 3 D) 6 E) 9 21. Sr(s) + P4(s) Sr3P2(s) A) 2 B) 3 C) 6 D) 12 E) 18 22. C2H6(g) + O2(g) CO2(g) + H2O(g) A) 4 B) 7 C) 8 D) 10 E) 14 14. Balance the following equation in standard form and determine the sum of the coefficients. FeO(s) + O2 (g ) Fe2O3 (s) A) B) C) D) E) 3 4 6 7 14 15. Consider the reaction represented by the unbalanced equation NH3 + O2 NO + H2O. For every 2.42 mol of NH3 that reacts, _______ mol of O2 is required. A) 2.42 B) 3.03 C) 9.68 D) 1.94 E) none of these Page 2 23. Li(s) + O2(g) Li2O(s) A) 1 B) 2 C) 3 D) 4 E) 5 29. When ethane (C2H6) is reacted with oxygen in the air, the products are carbon dioxide and water. This process requires __________ mol of oxygen for every 2.46 mol of ethane. A) 2.46 B) 6.15 C) 8.61 D) 17.22 E) none of these 24. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? KClO3 KCl + KClO4 A) 1 B) 2 C) 3 D) 4 E) 5 Use the following to answer questions 30-32: When the following equations are balanced using the smallest possible integers, what is the number in front of the underlined substance in each case? 25. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? NBr3 + NaOH N2 + NaBr + HOBr A) 1 B) 2 C) 3 D) 4 E) 5 26. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? C2H6 + O2 CO2 + H2O A) 1 B) 2 C) 4 D) 6 E) 7 30. Sb(s) + O2(g) Sb2O5(s) A) 1 B) 2 C) 4 D) 6 E) 12 31. C4H10(g) + O2(g) CO2(g) + H2O(g) A) 2 B) 4 C) 6 D) 8 E) 10 32. CH3OH(l) + O2(g) CO2(g) + H2O(g) A) 1 B) 2 C) 4 D) 6 E) 12 33. Which of the following statements about chemical reactions is false? A) In balancing a chemical equation, all subscripts must be conserved. B) When one coefficient is doubled, the rest of the coefficients in the balanced equation must also be doubled. C) The subscripts in a balanced equation tell us the number of atoms in a molecule. D) An individual coefficient in a balanced equation is meaningless. E) The phases in a chemical reaction tell us the nature of the reactants and products. 27. When the following equation is balanced using the smallest possible integers, what is the number in front of the substance in bold type? SiCl4 + H2O SiO2 + HCl A) 1 B) 2 C) 3 D) 4 E) 5 28. When table sugar is burned in air, carbon dioxide and water vapor are products, as shown by the following unbalanced chemical equation: C12H22O11(s) + O2(g) CO2(g) + H2O(g) How many moles of oxygen are required to react completely with 7.37 mol of sugar? A) 88.4 B) 7.37 C) 129 D) 177 E) none of these 34. When the equation Si(s) + HF(aq) SiF4(g) + H2(g) is balanced, what is the coefficient for HF? A) 0 B) 1 C) 2 D) 3 E) 4 Page 3 35. The factors that most commonly cause chemical reactions to occur are all the following except A) formation of a solid B) formation of a gas C) formation of water D) transfer of electrons E) a decrease in temperature 41. An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of lead (II) nitrate. The net ionic equation contains which of the following species (when balanced in standard form)? 36. A substance that, when dissolved in water, produces a solution that conducts electric current very efficiently is called A) a strong electrolyte B) a weak electrolyte C) a strong ion D) an electrical solute E) none of these 39. An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of lead (II) nitrate. What is the coefficient of the solid in the balanced equation (in standard form)? A) 1 B) 2 C) 3 D) 4 E) 6 40. An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of lead (II) nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)? B) 2NH 4 ( aq) 3Pb2 (aq) D) NO3 ( aq ) C) E) B) 2SO 24 (aq) C) 2NO3 ( aq) E) 38. An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of lead(II) nitrate. Identify the solid in the balanced equation. A) (NH4)2SO4 B) Pb(NO3)2 C) PbSO4 D) NH4NO3 E) There is no solid formed when the two solutions are mixed. 2SO 24 (aq) 2NH 4 ( aq) D) 37. When a precipitation reaction occurs, the ions that do not form the precipitate A) evaporate B) are cations only C) form a second insoluble compound in the solution D) are left dissolved in the solution E) none of these A) A) Na (aq) Page 4 Pb 2 (aq) NO3 (aq ) 42. Which drawing best represents the mixing of aqueous calcium chloride with aqueous potassium sulfate when they are mixed in stoichiometric amounts (neither reactant is limiting)? A) 43. An aqueous solution of sodium carbonate is reacted with an aqueous solution of calcium chloride. Identify the solid in the balanced equation. A) Na2CO3 B) CaCl2 C) NaCl D) CaCO3 E) There is no solid formed when the two solutions are mixed. 44. An aqueous solution of sodium carbonate is reacted with an aqueous solution of calcium chloride. What is the coefficient of the solid in the balanced equation (in standard form)? A) 5 B) 4 C) 3 D) 2 E) 1 B) 45. An aqueous solution of sodium carbonate is reacted with an aqueous solution of calcium chloride. The complete ionic equation contains which of the following species (when balanced in standard form)? C) B) Na (aq) 2CO32 (aq) C) 2Na (aq) D) Cl (aq) E) 3Ca 2 (aq) A) 46. An aqueous solution of sodium carbonate is reacted with an aqueous solution of calcium chloride. The net ionic equation contains which of the following species (when balanced in standard form)? D) E) A) CO32 ( aq) B) 2Na (aq) C) 2Cl (aq) D) Cl (aq) E) 2Ca 2 (aq) 47. The scientist who discovered the essential nature of acids through solution conductivity studies is A) Priestley B) Boyle C) Einstein D) Mendeleev E) Arrhenius Page 5 53. The reaction 2K(s) + Br2(l) 2KBr(s) is a(n) ______________ reaction. A) precipitation B) acid-base C) oxidation-reduction D) double-displacement E) single-replacement 48. When the following equation is balanced, what is the coefficient for H2O? Ca(OH)2(aq) + H3PO4(aq) Ca3(PO4)2(s) + H2O(l) A) 2 B) 3 C) 4 D) 6 E) 8 54. The reaction AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) is a(n) ______________ reaction. A) precipitation B) acid-base C) oxidation-reduction D) single-replacement E) none of these 49. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. Identify the solid in the balanced equation. A) KCl B) NaNO3 C) KNO3 D) NaCl E) There is no solid formed when the two solutions are mixed. 55. The equation 2C2H6 + 7O2 4CO2 + 6H2O is an oxidation-reduction reaction. True or false, and why? A) True; the carbon is oxidized, and the oxygen is reduced. B) True; the carbon is reduced, and the oxygen is oxidized. C) True; the carbon is oxidized, and the hydrogen is reduced. D) True; the oxygen is reduced, and the hydrogen is oxidized. E) False 50. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The molecular equation contains which one of the following terms (when balanced in standard form)? A) KCl(s) B) KNO3(aq) C) KNa(aq) D) ClNO3(aq) E) NaCl(s) 56. The reaction HCl(aq) + KOH(aq) H2O(l) + KCl(aq) is a(n) ______________ reaction. A) precipitation B) acid-base C) oxidation-reduction D) single-replacement E) none of these 51. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)? B) 2K (aq) 3NO3 ( aq ) C) Cl (aq) A) D) E) 57. How many electrons are transferred in the following oxidation-reduction reaction? Zn(s) + 2AgNO3(aq) Zn(NO3)2(aq) + 2Ag(s) A) 1 B) 2 C) 3 D) 4 E) 5 2Na (aq) 2KNO3 (aq) 52. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The net ionic equation contains which of the following species (when balanced in standard form)? B) 2K (aq) 3NO3 ( aq ) C) 2KNO3 (aq) A) D) E) 58. How many of the following are oxidation-reduction reactions? I. reaction of a metal with a nonmetal II. synthesis III. combustion IV. precipitation V. decomposition A) 1 B) 2 C) 3 D) 4 E) 5 2Na (aq) No net ionic equation exists for this reaction. Page 6 59. 65. The equation 2Al(s) + 2Br2(l) 2AlBr3(s) is a(n) ______________ reaction. A) oxidation-reduction and synthesis B) oxidation-reduction only C) synthesis only D) decomposition E) combustion In what type of reaction is water always a product? A) precipitation B) acid-base C) oxidation D) decomposition E) synthesis 60. Classify the following reaction: 2Mg(s) + O2(g) 2MgO(s) A) oxidation-reduction B) combustion C) synthesis D) two of the above E) a-c are all correct. 66. The equation 2Ag2O(s) 4Ag(s) + O2(g) is a(n) ______________ reaction. A) oxidation-reduction B) synthesis C) decomposition D) combustion E) two of these 61. Classify the following reaction: HNO3(aq) + KOH(aq) KNO3(aq) +H2O(l) A) oxidation-reduction B) combustion C) precipitation D) acid-base E) two of the above 67. 62. When the following equation is balanced in standard form, what is the coefficient in front of the underlined substance? C2H6(g) + O2(g) CO2(g) + H2O(l) A) 1 B) 2 C) 3 D) 4 E) 5 2. True or false? A catalyst is a substance that speeds up a reaction without being consumed. A) True B) False 3. True or false? A minimum energy called the activation energy is needed for a reaction to occur. A) True B) False 63. A reaction that involves a transfer of electrons is called a(n) ______________ reaction. A) precipitation B) acid-base C) oxidation-reduction D) double-displacement E) none of these 64. CH4(g) + 2O2(g) CO2(g) + 2H2O(g) A) oxidation-reduction B) synthesis C) decomposition D) combustion E) two of these 4. True or false? At equilibrium, the concentrations of all reactants and products are constant. A) True B) False 5. True or false? At equilibrium, the concentrations of all reactants and products are equal. A) True B) False Which of the following statements is not true? A) When a metal reacts with a nonmetal, an ionic compound is formed. B) A metal-nonmetal reaction can always be assumed to be an oxidation-reduction reaction. C) Two nonmetals can undergo an oxidation-reduction reaction. D) When two nonmetals react, the compound formed is ionic. E) A metal-nonmetal reaction involves electron transfer. 6. Given the reaction A(g) + B(g) C(g) + D(g). You have the gases A, B, C, and D at equilibrium. Upon adding gas A, the value of K A) increases because when A is added, more products are made, increasing the product-to-reactant ratio B) decreases because A is a reactant, so the product-toreactant ratio decreases C) does not change because A does not figure into the product-to-reactant ratio D) does not change as long as the temperature is constant E) depends on whether the reaction is endothermic or exothermic 7. Write the equilibrium expression for the reaction 3O2(g) 2O3(g) Page 7 8. Consider the general reaction aA + bB 11. cC + dD 2NO(g) + O2(g) Choose the correct equilibrium expression below. A) K B) K C) K D) E) C B) C) D) E) 10. F2(g) 2NO2(g) at a certain temperature, the equilibrium concentrations were found to be [NO2] = 5.1 10–3 M, [O2] = 1.0 10–2 M,and [NO] = 2.0 10–3 M. Calculate the value of the equilibrium constant from these data (delete units). A) 6.5 102 B) 12.7 104 C) 2.6 102 D) 1.5 10–3 E) none of these D [c ] [ d ] [a]A [b]B [C]c [D]d [A]a [B]b [A]a [B]b [C]c [D]d [a]A [b]B K C D [c ] [ d ] [cC][dD] K [aA][bB] 12. Write the equilibrium expression for the following reaction: S(s) + O2(g) SO2(g) [SO ] 2 [O ] 2 [O ] 2 B) K = [SO ]2 2 [SO ] 2 C) K = [O ]2 2 [SO ]2 2 D) K = [O ] 2 9. The correct equilibrium expression for the reaction of sulfur dioxide gas with oxygen gas to produce sulfur trioxide gas is A) For the reaction [SO ] 3 [SO ][O ] 2 2 [SO ]2 3 [SO ]2 [O ] 2 2 [SO ] 3 [SO ]2 [O ] 2 2 [O ][SO ]2 2 2 [SO ]2 3 A) K= E) none of these 13. Which of the following is an example of a homogeneous equilibrium reaction? A) 2CO(g) + O2(g) 2CO2(g) B) PCl5(s) PCl3(l) + Cl2(g) C) 2KClO3(s) 2KCl(s) + 3O2(g) D) CaCO3(s) CaO(s) + CO2(g) E) 6CO2(g) + 6H2O(g) C6H12O6(s) + 6O2(g) none of these For the reaction 14. Which of the following is an example of a heterogeneous equilibrium reaction? A) N2O4(g) 2NO2(g) B) H2(g) + F2(g) 2HF(g) C) C2H2(g) + 2Br2(g) C2H2Br4(g) D) N2(g) + 3H2(g) 2NH3(g) E) MgO(s) + CO2(g) MgCO3(s) 2F(g) at a particular temperature, the concentrations at equilibrium were observed to be [F2] = 2.2 10–2 mol/L and [F] = 2.0 10–4 mol/L. Calculate the value of the equilibrium constant from these data. (The units are deleted.) A) 4.4 10–2 B) 1.7 C) 5.5 105 D) 1.8 10–6 E) none of these Page 8 15. Choose the correct equilibrium expression for the following reaction. 2A(s) + 3B(l) C(aq) + 4D(aq) A) [A]2 [B]3 [C][D]4 B) [C] [D]4 C) D) E) 28. Consider the following equilibrium: 2H2(g) + X2(g) 2H2X(g) + energy The equilibrium expression is A) [2H2 X] [2H 2 ][X2 ] [2H 2 X] [2H 2 ] [X 2 ] [C][4D]4 [2A]2 [3B]3 [C][D]4 [A]2 [B]3 B) C) [H 2 X]2 [H 2 ]2 [X 2 ] none of these D) [H 2 X]2 [H 2 ]2 [X 2 ] E) none of these Use the following to answer questions 19-22: Consider the reaction 2H2(g) + O2(g) 2H2O(g) at some equilibrium position. Using the following choices, indicate what will happen if the changes below are made. 29. Consider the following equilibrium: 2H2(g) + X2(g) 2H2X(g) + energy Addition of X2 to this system at equilibrium A) will cause [H2] to decrease B) will cause [X2] to increase C) will cause [H2X] to increase D) will have no effect E) cannot possibly be carried out a. shifts to the left b. shifts to the right c. no change 19. Additional H2O(g) is injected into the reaction vessel. 20. Some H2(g) is removed from the reaction vessel. 21. The size of the reaction vessel is decreased. 22. Some He(g) is injected into the reaction vessel. 30. Consider the following equilibrium: 2H2(g) + X2(g) 2H2X(g) + energy Addition of argon to this system at equilibrium A) will cause [H2] to decrease B) will cause [X2] to increase C) will cause [H2X] to increase D) will have no effect E) cannot possibly be carried out Use the following to answer questions 23-27: Consider the reaction system CH4(g) + 2O2(g) CO2(g) + 2H2O(g) + energy, and use the following choices to describe what happens when the changes below are made to the system at equilibrium. 31. Consider the following equilibrium: 2H2(g) + X2(g) 2H2X(g) + energy Decreasing the volume of the container for this system at equilibrium will cause A) an increase in the amount of H2X B) an increase in the amounts of H2 and X2 C) an increase in the amount of H2 but not X2 D) no change E) X2 to dissociate a. shifts to the left b. shifts to the right c. no change 23. O2(g) is removed from the reaction vessel. 24. CO2(g) is removed from the reaction vessel. 25. He(g) is added to the reaction vessel. 26. The temperature is increased. 27. CH4(g) is added to the reaction vessel. Page 9 32. In the presence of ultraviolet light, the "inert" gas xenon (Xe) will react with fluorine (F2) gas to produce solid XeF4. What is the equilibrium expression for this reaction? A) B) C) D) E) 36. above A) B) C) D) E) [XeF4 ] [Xe][F2 ] [XeF4 ] [Xe][F2 ]2 1 [F2 ] 1 [Xe][F2 ]2 1 [Xe][F2 ] B) C) 38. Raising the pressure by decreasing the volume of the container A) will cause [A] to increase B) will cause [B] to increase C) will have no effect D) cannot be determined E) none of the above [H 2 ][I 2 ] [HI]2 39. Which of the following is true when the equilibrium constant for a reaction is relatively large? A) It will take a short time to reach equilibrium. B) It will take a long time to reach equilibrium. C) The equilibrium lies to the left. D) The equilbrium lies to the right. E) two of these [H 2 ][I 2 ] [HI]2 [HI] [H 2 ] D) [HI]2 [H 2 ][I 2 ] E) [HI]2 [H 2 ] will cause [A] to increase will cause [C] to increase will have no effect cannot be determined none of the above 37. Placing the equilibrium mixture in an ice bath (thus lowering the temperature) A) will cause [A] to increase B) will cause [B] to increase C) will have no effect D) cannot be determined E) none of the above 33. Consider the following equilibrium: H2(g) + I2(s) 2HI(g) The equilibrium expression is A) Addition of chemical B to an equilibrium mixture of the 40. Consider a system of four gases. The equilibrium concentration of each product is 2.7 M. The equilibrium concentrations of the reactants are equal. The equilibrium is shown here: A+B 34. True or false? The concentrations of pure solids or pure liquids involved in a chemical reaction are not included in the equilibrium expression for the reaction. A) True B) False C+D K = 2.6 What is the equilibrium concentration of gas A? A) 2.8 M B) 19.0 M C) 7.0 M D) 1.7 M E) 0.60 M Use the following to answer questions 35-38: 41. Given the equation A(g) B(g) + 2C(g). At a particular temperature, K = 1.4 105. For the reaction 2SO2(g) + O2(g) 35. If you mixed 1.2 mol B, 0.050 mol C, and 0.003 mol A in a 1-L container, in which direction would the reaction initially proceed? A) to the left B) to the right C) The mixture is in the equilibrium state. D) cannot tell from the information given 2SO3(g) at a certain temperature, the equilibrium concentrations were observed to be [SO2] = 0.733 M, [O2] = 7.50 10–2 M, and [SO3] = 0.650 M. Calculate the value of K for this system at this temperature. A) 11.8 B) 16.1 C) 7.69 D) 140 E) 10.5 Page 10 42. For the reaction CO(g) + H2O(g) 49. Given the solubility products (Ksp) BaSO4 1.5 10-9 CoS 5.0 10-22 PbSO4 1.3 10-2 AgBr 5.0 10-13 which of the following compounds is the most soluble (in mol/L)? A) BaSO4 B) CoS C) PbSO4 D) AgBr E) BaCO3 CO2(g) + H2(g) K = 3.88 at a certain temperature. If at this temperature in a certain experiment the equilibrium concentrations are [H2] = 1.9 M, [CO2] = 1.8 M, and [H2O] = 0.26 M, calculate [CO]. A) 0.29 M B) 1.9 M C) 3.7 M D) 3.4 M E) none of these 43. Write the balanced equation for the dissolving of PbCl2(s) in water. 50. The solubility of Fe(OH)2 in water at a certain temperature is 7.9 10–6 mol/L. The value of Ksp of Fe(OH)2 at this temperature is A) 7.9 10–6 B) 2.0 10–15 C) 4.9 10–16 D) 1.2 10–10 E) none of these 44. Write the balanced equation for the dissolving of Ag2S(s) in water. 45. Write the balanced equation for the dissolving of Fe3(PO4)2 in water. 46. The solubility of BaCO3(s) in water at a certain temperature is 3.8 10–5 mol/L. Calculate the value of Ksp for BaCO3(s) at this temperature. A) 3.8 10–5 B) 7.6 10–5 C) 1.4 10–9 D) 6.2 10–3 E) none of these 51. The molar solubility of PbI2 at a certain temperature is 1.5 10–3 M. Calculate the value of Ksp for PbI2. A) 1.5 10–3 B) 3.4 10–9 C) 1.4 10–8 D) 4.5 10–6 E) none of these 47. The solubility of Mg(OH)2(s) in water at a certain temperature is 1.0 10–4 mol/L. Calculate the value of Ksp for Mg(OH)2(s) at this temperature. A) 1.0 10–4 B) 1.0 10–12 C) 1.0 10–8 D) 4.0 10–12 E) none of these 52. Calculate the concentration of the silver ion in a saturated solution of silver chloride, AgCl (Ksp = 1.6 10-10). A) 5.4 10-4 B) 1.3 10-5 C) 1.6 10-10 D) 8.0 10-11 E) none of these 48. The Ksp for ZnS(s) is 2.9 10–22 at a certain temperature. The solubility of ZnS(s) in water at this temperature is A) 2.9 10–22 B) 1.7 10–11 C) 1.5 10–22 D) 5.8 10–22 E) none of these 53. The concentration of Ag+ in a saturated solution of Ag2CrO4 is 1.6 10-4 M. What is the Ksp value for Ag2CrO4? A) 2.0 10-12 B) 2.6 10-8 C) 4.1 10-12 D) 5.1 10-8 E) 1.6 10-11 54. The solubility of ZnS(s) in water at a certain temperature is 1.4 10–11 mol/L. The value of the Ksp of ZnS is A) 2.0 10–22 B) 1.4 10–11 C) 3.7 10–6 D) 7.0 10–12 E) 2.8 10–11 Page 11 55. The solubility in mol/L of Ag2CrO4 is 1.2 10–4 M at a certain temperature. What is the Ksp for this compound? A) 1.2 10–4 B) 1.7 10–12 C) 6.9 10–12 D) 2.9 10–8 E) 5.8 10–8 56. Silver chromate, Ag2CrO4, has a Ksp of 8.7 10–12 at a certain temperature. What is the solubility in mol/L of silver chromate? A) 1.3 10–4 B) 8.7 10–12 C) 2.2 10–12 D) 1.6 10–4 E) 4.7 10–24 57. The solubility of Cd(OH)2 in water at a certain temperature is 1.8 10–5 mol/L. The Ksp value for Cd(OH)2 is A) 2.3 10–14 B) 1.8 10–5 C) 5.8 10–15 D) 6.5 10–10 E) 3.2 10–10 Answer Key 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 21. 22. 23. 24. 25. 26. 27. 28. 29. 30. 31. 32. 33. C A B D D D D E C B E D A D B A B A C C C B B C B E D A C C D C A 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. 44. 45. 46. 47. 48. 49. 50. 51. 52. 53. 54. 55. 56. 57. 58. 59. 60. 61. 62. 63. 64. 65. 66. Page 12 E E A D C A B D B D E C A E D E B C E C A A B B D B E D D C D A E 67. E 2. 3. 4. 5. 6. 7. A A A B D 8. 9. 10. 11. 12. 13. 14. 15. B B D A A A E B 19. 20. 21. 22. 23. 24. 25. 26. 27. 28. a a b c a b c a b D K 29. 30. 31. 32. 33. 34. 35. 36. 37. 38. 39. 40. 41. 42. 43. 44. 45. 46. 47. 48. 49. 50. 51. 52. 53. 54. 55. 56. 57. [O3 ]2 [O 2 ]3 Page 13 A D A D E A B A D A D D E D PbCl2(s) Pb2+(aq) + Cl-(aq) Ag2S(s) 2Ag+(aq) + S2-(aq) Fe3(PO4)2(s) 3Fe2+(aq) + 2PO43-(aq) C D B C B C B A A C A A