Chem 1120 Pretest 3 Fall 2015

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1 Chem 1120 Pretest 3 Fall 2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of the following solubility product expressions is incorrect? a. Cu 2 S, K sp = [Cu + ][S 2 ] b. Co 2 S 3, K sp = [Co 3+ ] 2 [S 2 ] 3 c. Ni(CN) 2, K sp = [Ni 2+ ][CN ] 2 d. AuI, K sp = [Au + ][I ] e. Cr(OH) 3, K sp = [Cr 3+ ][OH ] 3 2. At 25 C, mole of Cd(OH) 2 dissolves to give 1.0 liter of saturated aqueous solution. What is the solubility product for Cd(OH) 2? a b c d e If X = the molar solubility (mol/l) of Ni(OH) 2, which of the following represents the correct relationship between the K sp and X, the molar solubility of Ni(OH) 2? a. K sp = 4 X 2 b. K sp = 4 X 3 c. K sp = 2 X 2 d. K sp = X 3 e. K sp = X 2 4. The K sp for magnesium arsenate is at 25 C. What is the molar solubility of Mg 3 (AsO 4 ) 2 at 25 C? a M b M c M d M e M 5. Which of the following has the lowest molar solubility in water at 25 C? a. Ni(CN) 2, K sp = b. ZnS, K sp = c. PbS, K sp = d. Co 3 (AsO 4 ) 2, K sp = e. CaF 2, K sp = Calculate the concentration of carbonate ion in a saturated solution of calcium carbonate to which calcium chloride has been added until [Ca 2+ ] = M at 25 C. K sp for CaCO 3 = a M b M c M

2 d M e M 7. The molar solubility of BaCO 3 is M at 25 C. What is the solubility product constant for BaCO 3? a b c d e A solution contains 0.05 M Au +, 0.05 M Cu +, and 0.05 M Ag + ions. When solid NaCl is added to the solution, what is the order in which the chloride salts will begin to precipitate? K sp(agcl) = , K sp(aucl) = , K sp(cucl) = a. AuCl > AgCl > CuCl b. AuCl > AgCl > NaCl c. AgCl > CuCl > AuCl d. CuCl > AgCl > AuCl e. NaCl > CuCl > AgCl 9. A solution is M in both Ag + and Au +. Some solid NaCl is added slowly until the second solid compound just begins to precipitate. What is the concentration of Au + ions at this point? K sp for AgCl = and for AuCl is a M b M c M d M e M 10. Solid silver nitrate is added slowly to a solution that is M in sodium chloride and M in sodium bromide. What % of the bromide ions remain in solution, i.e., unprecipitated, just before silver chloride begins to precipitate? K sp for AgCl = , K sp for AgBr = a. 0.18% b % c % d % e % 11. Calculate the concentration of F ions in saturated CaF 2 solution at 25 C. K sp = a M b M c M d M e M 12. AgCl would be least soluble at 25 C in. a. pure water b. 0.1 M CaCl 2 c. 0.1 M HCl

3 d. 0.1 M HNO 3 e. It is equally soluble in all of these substances. 13. Given the following values of K sp for four slightly soluble sulfides at 25 C. Sulfide K sp Sulfide K sp CdS PbS CuS MnS Which one of the following ions exists in the lowest concentration in a solution in which the sulfide ion concentration had been fixed at some (fairly large) constant value at 25 C? a. Cd 2+ b. Cu 2+ c. Pb 2+ d. Mn 2+ e. Cannot be answered without knowing the sulfide ion concentration. 14. K sp for lead fluoride is What is the molar solubility of PbF 2 in 0.10 M NaF? a M b M c M d M e M 15. If a solution is to be made M in Mg(NO 3 ) 2 and 0.20 M in aqueous NH 3, how many mol/l of NH 4 Cl are required to prevent the precipitation of Mg(OH) 2 at 25 C? The K b for aqueous NH 3 is and the K sp for Mg(OH) 2 is a b c d. 1.8 e The electrolysis of an aqueous sodium chloride solution using inert electrodes produces gaseous chlorine at one electrode. At the other electrode gaseous hydrogen is produced, and the solution becomes basic around the electrode. Which of the following is the equation for the cathode half-reaction in this electrolytic cell? a. 2Cl Cl 2 + 2e b. 2H 2 O + 2e H 2 + 2OH c. Cl 2 + 2e 2Cl d. H 2 + 2OH 2H 2 O + 2e e. none of these 17. An aqueous copper(ii) sulfate solution is electrolyzed for 45 minutes. A 3.2 ampere current is used. What mass of copper is produced? a g b. 1.9 g c. 2.8 g d. 4.6 g e. 5.5 g

4 Chapter 21 Values A table of standard electrode potentials is necessary for many of the following question(s). 18. Which of the following shorthand galvanic cell notations for the zinc copper standard cell is correct? Cu 2+ + Zn Zn 2+ + Cu a. Cu 2+ Cu Zn Zn 2+ b. Cu 2+ Cu Cu Cu 2+ c. Cu 2+ 2e 2e Zn d. Zn Zn 2+ Cu 2+ Cu e. Zn Cu 2+ Zn 2+ Cu 19. A voltaic cell is constructed by immersing a strip of copper metal in 1.0 M CuSO 4 solution and a strip of aluminum in 0.50 M Al 2 (SO 4 ) 3 solution. A wire and a salt bridge complete the circuit. The aluminum strip loses mass, and the concentration of aluminum ions in the solution increases. The copper electrode gains mass, and the concentration of copper ions decreases. What is the cell potential? a V b V c V d V e V 20. Calculate the cell potential for the following voltaic cell. Cr Cr 3+ ( M) Co 2+ ( M) Co a V b V c V d V e V 21. Which of the following statements about the operation of a standard galvanic cell made of a Cu/Cu 2+ half-cell and a Ag/Ag + half-cell is false? a. The mass of the copper electrode decreases. b. The electrons flow from the copper electrode to the silver electrode. c. The [Cu 2+ ] increases. d. Positive ions enter into the Ag/Ag + half-cell from the salt bridge. e. The copper electrode is positive. 22. Which one of the following reactions is spontaneous (in the direction given) under standard electrochemical conditions? a. Pb I Pb + I 2 b. Cu 2+ + Fe Cu + Fe 2+ c. 2Au + Pt 2+ 2Au + + Pt d. Mg Br Mg + Br 2 e. 2Hg + 2Cl + 2H + Hg 2 Cl 2 + H What is G 0 at 25 C for the reaction below? (F = 96,500 J/V mol e )

5 a kj b. 143 kj c. 597 kj d. 193 kj e kj Cu 2+ + Cd Cu + Cd The equilibrium constant, at 25 C, for the reaction below is What is E 0 for this reaction? NO 3 + 3H + + Cu Cu 2+ + HNO 2 + H 2 O a V b V c V d V e V 25. The K sp for Zn 3 (AsO 4 ) 2 is When 100 ml of M Zn 2+ is mixed with 50 ml of M AsO 3 4, which of the following statements is true? a. A precipitate forms, because Q sp > K sp. b. A precipitate forms, because Q sp < K sp. c. No precipitate forms, because Q sp > K sp. d. No precipitate forms, because Q sp < K sp. e. None of these statements is true. 26. The solubility of magnesium carbonate, MgCO 3, can be increased by acidifying the solution in which MgCO 3 is suspended. This is an example of dissolution via. a. formation of a weak electrolyte b. reduction of the anion c. oxidation of the anion d. formation of a complex ion e. changing an ion to another species which is not a weak electrolyte 27. Calculate the number of moles of ammonia needed to dissolve mole of silver chloride in ml of solution at 25 C. K sp for AgCl is and the dissociation constant for [Ag(NH 3 ) 2 ] + is a mole b mole c. 14 moles d mole e. 1.5 moles 28. In an electrolytic cell, the electrode that acts as a source of electrons to the solution is called the ; the chemical change that occurs at this electrode is called. a. anode; oxidation b. anode; reduction c. cathode; oxidation d. cathode; reduction e. Cannot answer unless we know the species being oxidized and reduced. 29. What product is formed at the anode when molten sodium chloride, NaCl, is electrolyzed using a Downs Cell?

6 a. O 2 b. Cl 2 c. NaOH d. H 2 e. Na metal 30. How long would a constant current of 4.5 amperes be required to flow in order to plate out 15 g of chromium from a chromium(iii) sulfate solution? a. 268 hr b. 309 hr c hr d hr e hr 31. Which of the following is not a feature of the lead storage battery? a. The electrolyte is hydrochloric acid. b. Lead is oxidized at the anode. c. PbO 2 is reduced at the cathode. d. Lead (II) sulfate forms during discharge and sticks to the electrodes. 32. Which one of the following formulas could represent a cycloalkane? a. C 2 H 6 b. C 3 H 8 c. C 4 H 10 d. C 6 H 12 e. C 7 H When carbon bonds in organic compounds, which of the following are true: a. Carbon makes 4 bonds. b. Carbon can form single, double or triple bonds. c. Carbon atoms can form branched chains. d. Carbon forms covalent bonds. e. All of these are true. 34. What is the molecular formula for heptane? a. C 7 H 14 b. C 7 H 12 c. C 9 H 18 d. C 7 H 16 e. C 9 H The correct IUPAC name for the compound shown below is. a. 2,2,4-trimethyl-7-propylnonane b. 7-ethyl-2,2,4-trimethyldecane

7 c. 3-propyl-6,8,8-trimethylnonane d. 4-ethyl-7,9,9-trimethylnonane e. 4-ethyl-7,9,9-trimethyldecane 36. Give the correct IUPAC name for the compound with the following structural formula. a. 2-ethyl-1,4-dimethylcyclopentane b. 3-ethyl-1,4-dimethylcyclohexane c. 1-ethyl-2,5-dimethylcyclohexane d. 2-ethyl-1,4-dimethylcyclohexane e. cyclic-2-ethyl-1,4-dimethylhexane 37. Which of the following is the correct formula for 2-methyl-1-butene? a. b. c. d. e. none of these 38. is an example of a(n). a. acid b. aldehyde c. phenol d. ketone e. ether 39. What is the name for the following compound? a. 4-ethyl-1,3,5-trimethylbenzene

8 b. 2-ethyl-1,3,5-trimethylbenzene c. 1,3,5-trimethyl-4-ethylbenzene d. 6-ethyl-1,3,5-trimethylbenzene e. 1-ethyl-2,4,6-trimethylbenzene 40. is an example of a(n). a. acid b. aldehyde c. phenol d. ketone e. ether 41. Which one of the following compounds is not an amine? a. (CH 3 ) 2 NH b. CH 3 CH 2 NH 2 c. C 6 H 5 NH 2 d. e. (CH 3 ) 3 N

9 Chem 1120 Pretest 3 Fall 2015 Answer Section MULTIPLE CHOICE 1. ANS: A PTS: 1 TOP: Solubility Product Constants 2. ANS: C PTS: 1 TOP: Determination of Solubility Product Constants 3. ANS: B PTS: 1 TOP: Determination of Solubility Product Constants 4. ANS: C PTS: 1 TOP: Uses of Solubility Product Constants 5. ANS: C PTS: 1 TOP: Uses of Solubility Product Constants 6. ANS: B PTS: 1 TOP: Uses of Solubility Product Constants 7. ANS: B PTS: 1 TOP: Determination of Solubility Product Constants 8. ANS: A PTS: 1 TOP: Fractional Precipitation 9. ANS: E PTS: 1 TOP: Fractional Precipitation 10. ANS: A PTS: 1 TOP: Fractional Precipitation 11. ANS: B PTS: 1 TOP: Uses of Solubility Product Constants 12. ANS: B PTS: 1 TOP: Uses of Solubility Product Constants 13. ANS: B PTS: 1 TOP: Uses of Solubility Product Constants 14. ANS: D PTS: 1 TOP: Uses of Solubility Product Constants 15. ANS: C PTS: 1 TOP: Simultaneous Equilibria Involving Slightly Soluble Compounds 16. ANS: B PTS: 1 TOP: The Electrolysis of Aqueous Salt Solutions 17. ANS: C PTS: 1 TOP: Counting Electrons: Coulometry and Faraday's Law of Electrolysis 18. ANS: D PTS: 1 TOP: The Zinc Copper Cell 19. ANS: B PTS: 1 TOP: Uses of Standard Electrode Potentials 20. ANS: A PTS: 1 TOP: The Nernst Equation 21. ANS: E PTS: 1 TOP: The Copper Silver Cell 22. ANS: B PTS: 1 TOP: Uses of Standard Electrode Potentials 23. ANS: B PTS: 1 TOP: The Relationship of E cell to Delta G and K 24. ANS: B PTS: 1 TOP: The Relationship of E cell to Delta G and K 25. ANS: A PTS: 1 TOP: Uses of Solubility Product Constants 26. ANS: A PTS: 1 TOP: Dissolving Precipitates 27. ANS: B PTS: 1 DIF: Harder Question TOP: Dissolving Precipitates 28. ANS: D PTS: 1 TOP: Electrodes 29. ANS: B PTS: 1 TOP: The Electrolysis of Molten Sodium Chloride (the Downs Cell) 30. ANS: C PTS: 1 TOP: Commercial Applications of Electrolytic Cells 31. ANS: A PTS: 1 TOP: The Lead Storage Battery 32. ANS: D PTS: 1 TOP: Alkanes and Cycloalkanes

10 33. ANS: E PTS: 1 TOP: Alkanes and Cycloalkanes 34. ANS: D PTS: 1 TOP: Alkanes and Cycloalkanes 35. ANS: B PTS: 1 TOP: Naming Saturated Hydrocarbons 36. ANS: D PTS: 1 TOP: Naming Saturated Hydrocarbons 37. ANS: A PTS: 1 TOP: Alkenes 38. ANS: B PTS: 1 TOP: Aldehydes and Ketones 39. ANS: B PTS: 1 TOP: Other Aromatic Hydrocarbons 40. ANS: D PTS: 1 TOP: Aldehydes and Ketones 41. ANS: D PTS: 1 TOP: Amines

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