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34 Cards in this Set
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5. What is/are the spectator ion(s) when a BaCl2 solution is combined with an H2SO4 solution?
A. Ba2+(aq), H+(aq) B. SO42-(aq), H+(aq) C. Cl-(aq) D. Cl-(aq), H+(aq) E. H+(aq) |
D. Cl-(aq), H+(aq)
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6. Which of the following are nonelectrolytes in water?
1 HF 2 ethanol, C2H5OH 3 C12H22O11 4 KClO3 5 Cu(NO3)2 A. ii and iii B. i, ii, and iii C. i, iv, and v D. iii E. ii |
A. ii and iii
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7. Which of the following is a weak base?
A. NaOH B. Ca(OH)2 C. NH3 D. RbOH E. Sr(OH)2 |
C. NH3
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8. Complete and balance the equation HClO4(aq) + Cu(OH)2(s)
A. 2HClO4(aq) + Cu(OH)2(s) à 2H2O(l) + Cu(ClO4)2(s) B. HClO4(aq) + Cu(OH)2(s) à H2O(l) + Cu+(aq) + ClO4-(aq) C. HClO4(aq) + Cu(OH)2(s) à H2O(l) + Cu2+(aq) + 2ClO4-(aq) D. 2HClO4(aq) + Cu(OH)2(s) à 2H2O(l) + Cu2+(aq) + 2ClO4-(aq) E. HClO4(aq) + Cu(OH)2(s) à H2O(l) + Cu(ClO4)2(s) |
D. 2HClO4(aq) + Cu(OH)2(s) à 2H2O(l) + Cu2+(aq) + 2ClO4-(aq)
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9. Which one of the following substances is predicted to be soluble in water?
A. AgCl B. PbSO4 C. Mg(OH)2 D. Mo(NO3)2 E. FeS |
D. Mo(NO3)2
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10. Write a balanced molecular equation for the reaction of hydrofluoric acid and calcium.
A. Ca(s) + 2HF(aq) à CaF2(aq) + 2H+(aq) B. Ca(s) + HF(aq) à CaF2(aq) + H2(g) C. Ca(s) + 2HF(aq) à CaF2(aq) + H2(g) D. Ca(s) + 2HF(aq) à CaF(aq) + H2(g) |
C. Ca(s) + 2HF(aq) à CaF2(aq) + H2(g)
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11. Complete and balance the equation HBr(aq) + Ca(OH)2(aq)
A. HBr(aq) + Ca(OH)2(aq) à H2O(l) + Ca+(aq) + Br-(aq) B. 2HBr(aq) + Ca(OH)2(aq) à 2H2O(l) + Ca2+(aq) + 2Br-(aq) C. HBr(aq) + Ca(OH)2(aq) à H2O(l) + Ca2+(aq) + 2Br-(aq) D. 2HBr(aq) + Ca(OH)2(aq) à 2H2O(l) + CaBr2(s) E. HBr(aq) + Ca(OH)2(aq) à H2O(l) + CaBr2(s) |
B. 2HBr(aq) + Ca(OH)2(aq) à 2H2O(l) + Ca2+(aq) + 2Br-(aq)
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12. A solution is made by mixing 30.0 mL of 8.00 M HCl, 100 mL of 2.00 M HCl, and enough water to make 200.0 mL of solution. What is the molarity of HCl in the final solution?
A. 0.455 M B. 1.20 M C. 2.20 M D. 0.440 M E. 10.00 M |
C. 2.20 M
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13. Which one of the following results in the formation of 0.200 M K2SO4 solution?
A. dilution of 250.0 mL of 1.00 M K2SO4 to 1.00 L B. dissolving 43.6 g of K2SO4 in water and diluting to a total volume of 250.0 mL C. diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL D. dissolving 20.2 g of K2SO4 in water and diluting to 250.0 mL, then diluting 25.0 mL of this solution to a total volume of 500.0 mL |
C. diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL
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14. Which reactions will not produce a precipitate from aqueous solution?
A. AgNO3 + KI B. FeSO4 + Ba(OH)2 C. Pb(NO3)2 + Na2CO3 D. ZnCl2 + (NH4)2S E. NaBr + Al2(SO4)2 |
E. NaBr + Al2(SO4)2
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15. Based on the activity series, which reaction below will not occur?
A. Mg(s) + 2HCl(aq) à MgCl2(aq) + H2(g) B. 2Ag(s) + 2HNO3(aq) à 2AgNO3(aq) + H2(g) C. 2Ni(s) + H2SO4(aq) à Ni2SO4(aq) + H2(g) D. 2Al(s) + 6HBr(aq) à 2AlBr3(aq) + 3H2(g) E. Zn(s) + 2HI(aq) à ZnI2(aq) + H2(g) |
B. 2Ag(s) + 2HNO3(aq) à 2AgNO3(aq) + H2(g)
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16. What volume of 0.125 M H2SO4 is required to completely precipitate all of the barium in 10.00 mL of a 0.150 M barium nitrate solution?
A. 12.0 mL B. 24.0 mL C. 6.00 mL D. 0.206 mL E. 0.010 mL |
A. 12.0 mL
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17. In the reaction Cl2(aq) + 2I-(aq) à 2Cl-(aq) + I2(aq), the species that is reduced is
A. Cl2. B. I-. C. Cl-. D. I2. |
A. Cl2.
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18. What volume of 0.125 M H2SO4 is required to neutralize 2.50 g of Ca(OH)2?
A. 0.270 mL B. 0.135 mL C. 135 mL D. 270 mL E. 540 mL |
D. 270 mL
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19. Which species is reduced in the reaction
A. 2MnO4-(aq) + 10I-(aq) + 16H+(aq) à 2Mn2+(aq) + 5I2(aq) + 8H2O(l)? B. MnO4- C. I- D. H+ E. Mn2+ F. I2 |
B. MnO4-
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20. Write a balanced net ionic equation for the reaction, if any, that may occur when the following pair is mixed: AgNO3(aq) and Na2CO3(aq)
A. There are only spectator ions. B. 2Na+(aq) + 2NO3-(aq) à2NaNO3(s) C. 2Ag+(aq) + CO32-(aq) àAg2CO3(s) D. 2Na+(aq) + 2Ag+(aq) + 2NO3-(aq) + CO32-(aq) àAg2CO3(s) + 2NaNO3(s) |
C. 2Ag+(aq) + CO32-(aq) àAg2CO3(s)
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21. Which of the following has the highest total concentration of ions?
A. 0.1 M CH3OH B. 0.1 M NaCl C. 0.05 M HBr D. 0.04 M (NH4)2SO4 E. 0.03 M Al2(SO4)3 |
B. 0.1 M NaCl
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When NaCl is added to a solution of (i) AgNO3, (ii) Pb(NO3)2, or (iii) Ca(NO3)2, in which case(s) does a precipitate form?
A. AgNO3 and Pb(NO3)2 only B. Pb(NO3)2 only C. in all three cases D. AgNO3 only E. Ca(NO3)2 only |
A. AgNO3 and Pb(NO3)2 only
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Write the net ionic reaction for the neutralization of HF by NaOH.
A. H+(aq) + OH-(aq) à H2O(l) B. HF(aq) + NaOH(aq) à NaF(aq) + H2O(l) C. HF(aq) + NaOH(aq) à Na+(aq) + F-(aq) + H2O(l) D. H+(aq) + NaOH(aq) à Na+(aq) + H2O(l) E. HF(aq) + OH-(aq) à F-(aq) + H2O(l) |
E. HF(aq) + OH-(aq) à F-(aq) + H2O(l)
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24. Which one of the following is not an electrolyte?
A. HCl B. Rb2SO4 C. Ar D. KOH |
C. Ar
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You want to perform an electrolysis experiment in which an electric current successfully passes through an aqueous solution. Which of the following substances would you add to a beaker of pure water to make this happen?
A. CO2 B. C2H5OH C. CCl4 D. NH4NO3 E. CH4 |
D. NH4NO3
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26. NH4Cl is a
A. strong base. B. strong acid. C. weak acid. D. weak base |
C. weak acid.
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Based on the activity series, which of the following reactions will occur?
(i)Al(s) + NiCl2(aq) (ii)Ag(s) + Pb(NO3)2(aq) (iii)Cr(s) + NiSO4(aq) A. i only B. ii only C. iii only D. i and ii E. i and iii |
D. i and ii
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What mass of ethanol, C2H5OH, is required to produce 300. mL of a 0.500 M solution?
A. 46.1 g B. 23.0 g C. 6.91 g D. 92.1 g E. 13.8 g |
C. 6.91 g
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29. If 5.20 g of a salt are found in 2.50 L of a 0.500 M solution, how many grams would be present in 2.50 L of a 1.50 M solution?
A. 5.20 g B. 10.4 g C. 15.6 g D. 1.73 g E. 7.8 g |
C. 15.6 g
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30. What is the mass of the precipitate formed when 12.0 mL of 0.150 M NaCl is added to 25.00 mL of a 0.0500 M AgNO3 solution?
A. 258 g B. 0.258 g C. 179 g D. 0.179 g E. 36.0 g |
D. 0.179 g
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31. A 25.0-g sample of garden compost was analyzed for chloride content. The sample was dissolved in water, and the chloride was precipitated as silver chloride. 1.58 g of dried precipitate was obtained. Calculate the mass percent of chloride in the sample.
A. 6.3 percent B. 4.8 percent C. 62 percent D. 3.1 percent E. 1.6 percent |
E. 1.6 percent
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32. Some sulfuric acid is spilled on a lab bench. It can be neutralized by sprinkling sodium bicarbonate on it and then mopping up the resultant solution. The sodium bicarbonate reacts with sulfuric acid in the following way:
2NaHCO3(s) + H2SO4(aq) Na2SO4(aq) + 2CO2(g) + 2 H2O(l) Sodium bicarbonate is added until the fizzing due to the formation of CO2(g) stops. If 35 mL of 6.0 M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid? A. 0.42 g B. 8.8 g C. 18 g D. 35 g E. 35280 g |
D. 35 g
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The minerals chalcocite (Cu2S) and malachite (Cu2CO3(OH)2) are two primary sources of copper. What is the oxidation state of copper in each of these minerals?
A. The oxidation state of copper in chalcocite is +1, and in malachite it is +2. B. The oxidation state of copper in chalcocite is +2, and in malachite it is +1. C. The oxidation state of copper in chalcocite is +2, and in malachite it is +2. D. The oxidation state of copper in chalcocite is +1, and in malachite it is +1. E. The oxidation state of copper in chalcocite is +2, and in malachite it is +4. |
A. The oxidation state of copper in chalcocite is +1, and in malachite it is +2.
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46. What is the molarity of the salt produced in the reaction of 200 mL of 0.100 M HCl with 100 mL of 0.500 M KOH?
A. 0.0325 M B. 0.0472 M C. 0.0667 M D. 0.0864 M E. 0.0935 M |
C. 0.0667 M
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55. A 0.6745 gram sample of KHP reacts with 41.75 mL of KOH solution for complete neutralization. What is the molarity of the KOH solution? (Molecular weight of KHP = 204 g/mol. KHP has one acidic hydrogen.)
A. 0.158 M B. 0.099 M C. 0.139 M D. 0.079 M E. 0.061 M |
D. 0.079 M
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59. In which of the following does nitrogen have an oxidation number of -3?
1 NH3 2 Li3N 3 (NH4)2HPO4 4 NO3 A. all of the above B. b only C. a&c D. a,b&c |
D. a,b&c
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63. When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. The balanced equation for this reaction is _________.
A. KH + BaCl à KCl + BaH B. KOH + BaCl2 à KCl2 + BaOH C. 2KOH + BaCl2 à 2KCl + Ba(OH)2 D. KOH + BaCl à KCl + BaOH E. 2KOH + 2BaCl2 à 2KCl2 + 2Ba(OH)2 |
C. 2KOH + BaCl2 à 2KCl + Ba(OH)2
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64. In the above problem, identify the precipitate.
A. potassium hydroxide B. barium chloride C. potassium chloride D. barium hydroxide E. no precipitate is formed |
D. barium hydroxide
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