Chapter 4 1 Cobalt More Active Than nickel But Less Active

Chemistry: The Central Science, 13e (Brown et al.)

Chapter 4 Aqueous Reactions and Solution Stoichiometry

4.1 Multiple Choice Questions

1) Of the species below, only ________ is not an electrolyte.

A) HCl

B) Rb2SO4

C) Ar

D) KOH

E) NaCl

2) The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is

________.

A) 2H+ (aq) + 2OH– (aq) → 2H2O (l)

B) 2H+ (aq) + 2KOH (aq) → 2H2O (l) + 2K+ (aq)

C) H2SO4 (aq) + 2OH– (aq) → 2H2O (l) + SO42- (aq)

D) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (s)

E) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq)

3) Aqueous potassium chloride will react with which one of the following in an exchange (metathesis)

reaction?

A) calcium nitrate

B) sodium bromide

C) lead nitrate

D) barium nitrate

E) sodium chloride

4) Aqueous solutions of a compound did not form precipitates with Cl–, Br–, I–, SO42-, CO32–, PO43-,

OH–, or S2-. This highly water-soluble compound produced the foul-smelling gas H2S when the solution

was acidified. This compound is ________.

A) Pb(NO3)2

B) (NH4)2S

C) KBr

D) Li2CO3

E) AgNO3

5) The net ionic equation for formation of an aqueous solution of NiI2 accompanied by evolution of CO2

gas via mixing solid NiCO3 and aqueous hydriodic acid is ________.

A) 2NiCO3 (s) + HI (aq) → 2H2O (l) + CO2 (g) + 2Ni2+ (aq)

B) NiCO3 (s) + I– (aq) → 2H2O (l) + CO2 (g) + Ni2+ (aq) + HI (aq)

C) NiCO3 (s) + 2H+ (aq) → H2O (l) + CO2 (g) + Ni2+ (aq)

D) NiCO3 (s) + 2HI (aq) → 2H2O (l) + CO2 (g) + NiI2 (aq)

E) NiCO3 (s) + 2HI (aq) → H2O (l) + CO2 (g) + Ni2+ (aq) + 2I– (aq)

6) The net ionic equation for formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3 and

aqueous nitric acid is ________.

A) Al(OH)3 (s) + 3HNO3 (aq) → 3H2O (l) + Al(NO3)3 (aq)

B) Al(OH)3 (s) + 3NO3– (aq) → 3OH– (aq) + Al(NO3)3 (aq)

C) Al(OH)3 (s) + 3NO3– (aq) → 3OH– (aq) + Al(NO3)3 (s)

D) Al(OH)3 (s) + 3H+ (aq) → 3H2O (l) + Al3+ (aq)

E) Al(OH)3 (s) + 3HNO3 (aq) → 3H2O (l) + Al3+ (aq) + NO3– (aq)

7) Which of the following is insoluble in water at 25 °C?

A) Mg3(PO4)2

B) Na2S

C) (NH4)2CO3

D) Ca(OH)2

E) Ba(C2H3O2)2

8) When aqueous solutions of ________ are mixed, a precipitate forms.

A) NiBr2 and AgNO3

B) NaI and KBr

C) K2SO4 and CrCl3

D) KOH and Ba(NO3)2

E) Li2CO3 and CsI

9) Which one of the following compounds is insoluble in water?

A) Na2CO3

B) K2SO4

C) Fe(NO3)3

D) ZnS

E) AgNO3

10) Which one of the following compounds is insoluble in water?

A) K2SO4

B) Ca(C2H3O2)2

C) MgC2O4

D) ZnCl2

E) Mn(NO3)2

11) Which combination will produce a precipitate?

A) NaC2H3O2 (aq) and HCl (aq)

B) NaOH (aq) and HCl (aq)

C) AgNO3(aq) and Ca(C2H3O2)2 (aq)

D) KOH (aq) and Mg(NO3)2 (aq)

E) NaF (aq) and HCl (aq)

12) Which combination will produce a precipitate?

A) NH4OH (aq) and HCl (aq)

B) AgNO3 (aq) and Ca(C2H3O2)2 (aq)

C) NaOH (aq) and HCl (aq)

D) NaCl (aq) and HC2H3O2 (aq)

E) NaOH (aq) and Fe(NO3)2 (aq)

13) Which combination will produce a precipitate?

A) Pb(NO3)2 (aq) and HCl (aq)

B) Cu(NO3)2 (aq) and KC2H3O2 (aq)

C) KOH (aq) and HNO3 (aq)

D) AgC2H3O2 (aq) and HC2H3O2 (aq)

E) NaOH (aq) and Sr(NO3)2 (aq)

14) With which of the following will the ammonium ion form an insoluble salt?

A) chloride

B) sulfate

C) carbonate

D) sulfate and carbonate

E) none of the above

15) The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide

is ________.

A) H+ (aq) + HSO4– (aq) + 2OH– (aq) → 2H2O (l) + SO42- (aq)

B) H+ (aq) + HSO4– (aq) + 2Na+ (aq) + 2OH– (aq) → 2H2O (l) + 2Na+ (aq) + SO42-(aq)

C) SO42- (aq) + 2Na+ (aq) → 2Na+ (aq) + SO42-(aq)

D) H+ (aq) + OH– (aq) → H2O( l)

E) 2H+ (aq) + SO42- (aq) + 2Na+ (aq) + 2OH– (aq) → 2H2O (l) + 2Na+ (aq) + SO42- (aq)

16) The net ionic equation for the reaction between aqueous nitric acid and aqueous sodium hydroxide is

________.

A) H+ (aq) + HNO3 (aq) + 2OH– (aq) → 2H2O (l) + NO3– (aq)

B) HNO3 (aq) + NaOH (aq) → NaNO3 (aq) + H2O (l)

C) H+ (aq) + OH– (aq) → H2O (l)

D) HNO3 (aq) + OH– (aq) → NO3– (aq) + H2O (l)

E) H+ (aq) + Na+ (aq) + OH– (aq) → H2O (l) + Na+ (aq)

17) The reaction between strontium hydroxide and chloric acid produces ________.

A) a molecular compound and a weak electrolyte

B) two weak electrolytes

C) two strong electrolytes

D) a molecular compound and a strong electrolyte

E) two molecular compounds

18) Which one of the following is a diprotic acid?

A) nitric acid

B) chloric acid

C) phosphoric acid

D) hydrofluoric acid

E) sulfuric acid

19) Which one of the following is a triprotic acid?

A) nitric acid

B) chloric acid

C) phosphoric acid

D) hydrofluoric acid

E) sulfuric acid

20) Which one of the following is a weak acid?

A) HNO3

B) HCl

C) HI

D) HF

E) HClO4

21) Which of the following are weak acids?

A) HF, HBr

B) HI, HNO3, HBr

C) HI, HF

D) HF

E) none of the above

22) A compound was found to be soluble in water. It was also found that addition of acid to an aqueous

solution of this compound resulted in the formation of carbon dioxide. Which one of the following

cations would form a precipitate when added to an aqueous solution of this compound?

A) NH4+

B) K+

C) Cr3+

D) Rb+

E) Na+

23) The balanced reaction between aqueous potassium hydroxide and aqueous acetic acid is ________.

A) KOH (aq) + HC2H3O2 (aq) → OH– (l) + HC2H3O2+ (aq) + K (s)

B) KOH (aq) + HC2H3O2 (aq) → H2O (l) + KC2H3O2 (aq)

C) KOH (aq) + HC2H3O2 (aq) → H2C2H3O3 (aq) + K (s)

D) KOH (aq) + HC2H3O2 (aq) → KC2H3O3 (aq) + H2 (g)

E) KOH (aq) + HC2H3O2 (aq) → H2KC2H3O (aq) + O2 (g)

24) The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is ________.

A) HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + H2 (g)

B) HNO3 (aq) + Sr(OH)2 (aq) → H2O (l) + Sr(NO3)2 (aq)

C) HNO3 (aq) + SrOH (aq) → H2O (l) + SrNO3 (aq)

D) 2HNO3 (aq) + Sr(OH)2 (aq) → 2H2O (l) + Sr(NO3)2 (aq)

E) 2HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2(aq) + 2H2 (g)

25) In which reaction does the oxidation number of oxygen increase?

A) Ba(NO3)2 (aq) + K2SO4 (aq) → BaSO4 (s) + 2KNO3 (aq)

B) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)

C) MgO (s) + H2O (l) → Mg(OH)2 (s)

D) 2SO2 (g) + O2 (g) → 2SO3 (g)

E) 2H2O (l) → 2H2 (g) + O2 (g)

26) In which reaction does the oxidation number of hydrogen change?

A) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)

B) 2Na (s) + 2H2O (l) → 2NaOH (aq) + H2 (g)

C) CaO (s) + H2O (l) → Ca(OH)2 (s)

D) 2HClO4 (aq) + CaCO3 (s) → Ca(ClO4)2 (aq) + H2O (l) + CO2 (g)

E) SO2 (g) + H2O (l) → H2SO3 (aq)

27) Which compound has the atom with the highest oxidation number?

A) CaS

B) Na3N

C) MgSO3

D) Al(NO2)3

E) NH4Cl

28) Of the choices below, which would be the best for the lining of a tank intended for use in storage of

hydrochloric acid?

A) copper

B) zinc

C) nickel

D) iron

E) tin

29) Which of these metals will be oxidized by the ions of cobalt?

A) nickel

B) tin

C) iron

D) copper

E) silver

30) Which of these metals will be oxidized by the ions of aluminum?

A) magnesium

B) zinc

C) chromium

D) iron

E) nickel

31) One method for removal of metal ions from a solution is to convert the metal to its elemental form so

it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution?

A) zinc

B) cobalt

C) lead

D) copper

E) none of these

32) Of the reactions below, only ________ is not spontaneous.

A) Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2(g)

B) 2Ag (s) + 2HNO3 (aq) → 2AgNO3 (aq) + H2 (g)

C) 2Ni (s) + H2SO4 (aq) → Ni2SO4 (aq) + H2 (g)

D) 2Al (s) + 6HBr (aq) → 2AlBr3 (aq) + 3H2 (g)

E) Zn (s) + 2HI (aq) → ZnI2(aq) + H2 (g)

33) Based on the activity series, which one of the reactions below will occur?

A) Zn (s) + MnI2 (aq) → ZnI2 (aq) + Mn (s)

B) SnCl2 (aq) + Cu (s) → Sn (s) + CuCl2 (aq)

C) 2AgNO3 (aq) + Pb (s) → 2Ag (s) + Pb(NO3)2 (aq)

D) 3Hg (l) + 2Cr(NO3)3 (aq) → 3Hg(NO3)2 + 2Cr (s)

E) 3FeBr2 (aq) + 2Au (s) → 3Fe (s) + 2AuBr3 (aq)

34) Based on the activity series, which one of the reactions below will occur?

A) Fe (s) + ZnCl2 (aq) → FeCl2 (aq) + Zn (s)

B) Mn (s) + NiCl2 (aq) → MnCl2 (aq) + Ni (s)

C) Pb (s) + NiI2 (aq) → PbI2 (aq) + Ni (s)

D) SnBr2 (aq) + Cu (s) → CuBr2 (aq) + Sn (s)

E) None of the reactions will occur.

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35) The net ionic equation for the dissolution of zinc metal in aqueous hydrobromic acid is ________.

A) Zn (s) + 2Br– (aq) → ZnBr2 (aq)

B) Zn (s) + 2HBr (aq) → ZnBr2 (aq) + 2H+ (aq)

C) Zn (s) + 2HBr (aq) → ZnBr2 (s) + 2H+ (aq)

D) Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g)

E) 2Zn (s) + H+ (aq) → 2Zn2+ (aq) + H2 (g)

36) Sodium does not occur in nature as Na (s) because ________.

A) it is easily reduced to Na–

B) it is easily oxidized to Na+

C) it reacts with water with great difficulty

D) it is easily replaced by silver in its ores

E) it undergoes a disproportionation reaction to Na– and Na+

37) Zinc is more active than cobalt and iron but less active than aluminum. Cobalt is more active than

nickel but less active than iron. Which of the following correctly lists the elements in order of increasing

activity?

A) Co < Ni < Fe < Zn < Al

B) Ni < Fe < Co < Zn < Al

C) Ni < Co < Fe < Zn < Al

D) Fe < Ni < Co < Al < Zn

E) Zn < Al < Co < Ni < Fe

38) Oxidation is the ________ and reduction is the ________.

A) gain of oxygen, loss of electrons

B) loss of oxygen, gain of electrons

C) loss of electrons, gain of electrons

D) gain of oxygen, loss of mass

E) gain of electrons, loss of electrons

39) Oxidation and ________ mean essentially the same thing.

A) activity

B) reduction

C) metathesis

D) decomposition

E) corrosion

40) Oxidation cannot occur without ________.

A) acid

B) oxygen

C) water

D) air

E) reduction

41) Which of the following is an oxidationfireduction reaction?

A) Cu (s) + 2AgNO3 (aq) → 2Ag (s) + Cu(NO3)2 (aq)

B) HCl (aq) + NaOH (aq) → H2O (l) + NaCl (aq)

C) AgNO3 (aq) + HCl (aq) → AgCl (s) + HNO3 (aq)

D) Ba(C2H3O2)2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2NaC2H3O2(aq)

E) H2CO3 (aq) + Ca(NO3)2 (aq) → 2HNO3 (aq) + CaCO3 (s)

42) Which of the following reactions will not occur as written?

A) Zn (s) + Pb(NO3)2 (aq) → Pb (s) + Zn(NO3)2 (aq)

B) Mg (s) + Ca(OH)2 (aq) → Ca (s) + Mg(OH)2 (aq)

C) Sn (s) + 2AgNO3 (aq) → 2Ag (s) + Sn(NO3)2 (aq)

D) Co (s) + 2AgCl (aq) → 2Ag (s) + CoCl2 (aq)

E) Co (s) + 2HI (aq) → H2 (g) + CoI2 (aq)

43) Which one of the following is a correct expression for molarity?

A) mol solute/L solvent

B) mol solute/mL solvent

C) mmol solute/mL solution

D) mol solute/kg solvent

E) μmol solute/L solution

44) Which one of the following is not true concerning 2.00 L of 0.100 M solution of Ca3(PO4)2?

A) This solution contains 0.200 mol of Ca3(PO4)2.

B) This solution contains 0.800 mol of oxygen atoms.

C) 1.00 L of this solution is required to furnish 0.300 mol of Ca2+ ions.

D) There are 6.02 × 1022 phosphorus atoms in 500.0 mL of this solution.

E) This solution contains 0.600 mol of Ca2+.

45) A 0.200 M K2SO4 solution is produced by ________.

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

E) dilution of 1.00 mL of 250 M K2SO3 to 1.00 L

46) Which solution has the same number of moles of NaOH as 50.0 mL of 0.100 M solution of NaOH?

A) 20.0 mL of 0.200 M solution of NaOH

B) 25.0 mL of 0.175 M solution of NaOH

C) 30.0 mL of 0.145 M solution of NaOH

D) 50.0 mL of 0.125 M solution of NaOH

E) 100.0 mL of 0.0500 M solution of NaOH

47) Which solution has the same number of moles of KCl as 75.00 mL of 0.250 M solution of KCl?

A) 20.0 mL of 0.200 M solution of KCl

B) 25.0 mL of 0.175 M solution of KCl

C) 129 mL of 0.145 M solution of KCl

D) 50.0 mL of 0.125 M solution of KCl

E) 100 mL of 0.0500 M solution of KCl

48) What are the respective concentrations (M) of Fe3+ and I– afforded by dissolving 0.200 mol FeI3 in

water and diluting to 725 mL?

A) 0.276 and 0.828

B) 0.828 and 0.276

C) 0.276 and 0.276

D) 0.145 and 0.435

E) 0.145 and 0.0483

49) What are the respective concentrations (M) of Mg2+ and C2H3O2– afforded by dissolving 0.600 mol

Mg(C2H3O2)2 in water and diluting to 135 mL?

A) 0.444 and 0.889

B) 0.0444 and 0.0889

C) 0..889 and 0.444

D) 0.444 and 0.444

E) 4.44 and 8.89

50) A tenfold dilution of a sample solution can be obtained by taking ________.

A) 1 part sample and 9 parts solvent

B) 1 part sample and 10 parts solvent

C) 9 parts sample and 1 part solvent

D) 10 parts sample and 1 part solvent

E) 99 parts sample and 1 part solvent

51) Mixing 10.00 mL of an aqueous solution with 10.00 mL of water represents a ________.

A) crystallization

B) neutralization

C) twofold dilution

D) tenfold dilution

E) titration

52) You are given two clear solutions of the same unknown monoprotic acid, but with different

concentrations. Which statement is true?

A) There is no chemical method designed to tell the two solutions apart.

B) It would take more base solution (per milliliter of the unknown solution) to neutralize the more

concentrated solution.

C) A smaller volume of the less concentrated solution contains the same number of moles of the acid

compared to the more concentrated solution.

D) If the same volume of each sample was taken, then more base solution would be required to neutralize

the one with lower concentration.

E) The product of concentration and volume of the less concentrated solution equals the product of

concentration and volume of the more concentrated solution.

53) A 0.100 M solution of ________ will contain the highest concentration of potassium ions.

A) potassium phosphate

B) potassium hydrogen carbonate

C) potassium hypochlorite

D) potassium iodide

E) potassium oxide

54) Which solution contains the largest number of moles of chloride ions?

A) 10.0 mL of 0.500 M BaCl2

B) 4.00 mL of 1.000 M NaCl

C) 7.50 mL of 0.500 M FeCl3

D) 25.00 mL of 0.400 M KCl

E) 30.00 mL of 0.100 M CaCl2

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55) What volume (mL) of a concentrated solution of magnesium chloride (9.00 M) must be diluted to 350.

mL to make a 2.75 M solution of magnesium chloride?

A) 2.75

B) 50.0

C) 45.0

D) 107

E) 350

56) What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200.0

mL to make a 0.880 M solution of sodium hydroxide?

A) 2.64

B) 176

C) 26.4

D) 29.3

E) 50.0

57) What mass (g) of potassium chloride is contained in 430.0 mL of a potassium chloride solution that

has a chloride ion concentration of 0.193 M?

A) 0.0643

B) 0.0830

C) 12.37

D) 0.386

E) 6.19

58) What volume (L) of 0.250 M HNO3 is required to neutralize a solution prepared by dissolving 17.5 g

of NaOH in 350 mL of water?

A) 50.0

B) 0.44

C) 1.75

D) 0.070

E) 1.75 ×

59) An aliquot (28.7 mL) of a KOH solution required 31.3 mL of 0.118 M HCl for neutralization. What

mass (g) of KOH was in the original sample?

A) 1.64

B) 7.28

C) 0.173

D) 0.207

E) 0.414

60) The point in a titration at which the indicator changes is called the ________.

A) setpoint

B) indicator point

C) standard point

D) end point

E) volumetric point

61) Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for

neutralization?

A) 10.0 mL of 0.0500 M phosphoric acid

B) 20.0 mL of 0.0500 M nitric acid

C) 5.0 mL of 0.0100 M sulfuric acid

D) 15.0 mL of 0.0500 M hydrobromic acid

E) 10.0 mL of 0.0500 M perchloric acid

62) Which one of the following substances is produced during the reaction of an acid with a metal

hydroxide?

A) H2

B) H2O

C) CO2

D) NaOH

E) O2

63) What volume (mL) of 7.48 × 10-2 M perchloric acid can be neutralized with 115 mL of 0.244 M sodium

hydroxide?

A) 125

B) 8.60

C) 188

D) 750

E) 375

64) ________ is an oxidation reaction.

A) Ice melting in a soft drink

B) Table salt dissolving in water for cooking vegetables

C) Rusting of iron

D) The reaction of sodium chloride with lead nitrate to form lead chloride and sodium nitrate

E) Neutralization of HCl by NaOH

4.2 Bimodal Questions

1) A strong electrolyte is one that ________ completely in solution.

A) reacts

B) associates

C) disappears

D) ionizes

2) A weak electrolyte exists predominantly as ________ in solution.

A) atoms

B) ions

C) molecules

D) electrons

E) an isotope

3) Which of the following are strong electrolytes?

HCl

HC2H3O2

NH3

KCl

A) HCl, KCl

B) HCl, NH3, KCl

C) HCl, HC2H3O2, NH3, KCl

D) HCl, HC2H3O2, KCl

E) HC2H3O2, KCl

4) Which of the following are weak electrolytes?

HNO3

HF

NH3

LiBr

A) HNO3, LiBr

B) HNO3, HF, NH3, LiBr

C) HF, LiBr

D) HF, NH3

E) HNO3, NH3, LiBr

5) What are the spectator ions in the reaction between KOH (aq) and HNO3 (aq)?

A) K+ and H+

B) H+ and OH–

C) K+ and NO3–

D) H+ and NO3–

E) OH– only

6) What are the spectator ions in the reaction between KCl (aq) and AgNO3 (aq)?

A) K+ and Ag+

B) Ag+ and Cl–

C) K+ and NO3–

D) Ag+ and NO3–

E) K+ only

7) What are the spectator ions in the reaction between Mg(OH)2 (aq) and HCl (aq)?

A) Mg+2 and H+

B) H+ and OH–

C) Mg+2 and Cl–

D) H+ and Cl–

E) OH– only

8) The net ionic equation for the reaction between aqueous solutions of HF and KOH is ________.

A) HF + KOH → H2O + K+ + F–

B) HF + OH– → H2O + F–

C) HF + K+ + OH– → H2O + KF

D) H+ + OH– → H2O

E) H+ + F– + K+ + OH– → H2O + K+ + F–

9) Combining aqueous solutions of BaI2 and Na2SO4 affords a precipitate of BaSO4. Which ions are

spectator ions in the reaction?

A) Ba2+ only

B) Na+ only

C) Ba2+ and SO42–

D) Na+ and I–

E) SO42- and I–

10) Which ions are spectator ions in the formation of a precipitate of AgCl via combining aqueous

solutions of CoCl2 and AgNO3?

A) Co2+ and NO3–

B) NO3– and Cl–

C) Co2+ and Ag+

D) Cl–

E) NO3–

11) The balanced net ionic equation for precipitation of CaCO3 when aqueous solutions of Na2CO3 and

CaCl2 are mixed is ________.

A) 2Na+ (aq) + CO32– (aq) → Na2CO3 (aq)

B) 2Na+ (aq) + 2Cl– (aq) → 2NaCl (aq)

C) Na+ (aq) + Cl– (aq) → NaCl (aq)

D) Ca+(aq) + CO32- (aq) → CaCO3 (s)

E) Na2CO3 (aq) + Ca (aq) → 2NaCl (aq) + CaCO3 (s)