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)

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

A) Al(OH)3 (s) + 3HNO3 (aq) → 3H2O (l) + Al(NO3)3 (aq)2+ (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

A) Mg3(PO4)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

A) NiBr2 and AgNO3

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

A) Na2CO3

B) K2SO4

C) Fe(NO3)3

D) ZnS

E) AgNO3

D) ZnS

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

C) MgC2O4

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)

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

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)

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

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)

D) H+ (aq) + OH- (aq) → H2O( l)

16) 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

D) a molecular compound and a strong electrolyte

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

A) nitric acid

B) chloric acid

C) phosphoric acid

D) hydrofluoric acid

E) sulfuric acid

E) sulfuric acid

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

A) nitric acid

B) chloric acid

C) phosphoric acid

D) hydrofluoric acid

E) sulfuric acid

C) phosphoric acid

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

A) HNO3

B) HCl

C) HI

D) HF

E) HClO4

D) HF

20) 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+

C) Cr3+

21) 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)

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

22) 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)

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

23) 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)

E) 2H2O (l) → 2H2 (g) + O2 (g)

24) 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)

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

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

A) CaS

B) Na3N

C) MgSO3

D) Al(NO2)3

E) NH4Cl

C) MgSO3

26) 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

A) copper

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

A) nickel

B) tin

C) iron

D) copper

E) silver

C) iron

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

A) magnesium

B) zinc

C) chromium

D) iron

E) nickel

A) magnesium

29) 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

E) none of these

30) 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)

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

31) 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)

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

32) 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.

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

33) 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)

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

34) 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+

B) it is easily oxidized to Na+

35) 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

C) Ni < Co < Fe < Zn < Al

36) 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

C) loss of electrons, gain of electrons

37) Oxidation and ________ mean essentially the same thing.

A) activity

B) reduction

C) metathesis

D) decomposition

E) corrosion

E) corrosion

38) Oxidation cannot occur without ________.

A) acid

B) oxygen

C) water

D) air

E) reduction

E) reduction

39) Which of the following is an oxidation-reduction 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)

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

40) 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)

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

41) 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

C) mmol solute/mL solution

42) 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+.

B) This solution contains 0.800 mol of oxygen atoms.

43) 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

C) diluting 20.0 mL of 5.00 M K2SO4 solution to 500.0 mL

44) 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

E) 100.0 mL of 0.0500 M solution of NaOH

45) 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

C) 129 mL of 0.145 M solution of KCl

46) 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

A) 0.276 and 0.828

FeI₃-> Fe³⁺ + 3I^-

[FeI₃]= .200mol/.725L=0.276m

[I-]= 3 x 0.276= .828m

47) 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

E) 4.44 and 8.89

48) 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

A) 1 part sample and 9 parts solvent

49) 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

C) twofold dilution

50) 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.

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

51) 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

A) potassium phosphate

52) 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

C) 7.50 mL of 0.500 M FeCl3

53) 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

D) 107

54) 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

D) 29.3

55) 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

E) 6.19

56) 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 × 10^-3

C) 1.75

57) 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

D) 0.207