Answer at the bottom of the page
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) → 2 H2O (l)
B) 2H+ (aq) + 2KOH (aq) → 2 H2O (l) + 2K+ (aq)
C) H2SO4 (aq) + 2OH- (aq) → 2 H2O (l) + SO42- (aq)
D) H2SO4 (aq) + 2KOH (aq) → 2 H2O (l) + K2SO4 (s)
E) H2SO4 (aq) + 2KOH (aq) → 2 H2O (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) → 2 H2O (l) + CO2 (g) + 2Ni2+ (aq)
B) NiCO3 (s) + I- (aq) → 2 H2O (l) + CO2 (g) + Ni2+ (aq) + HI (aq)
C) NiCO3 (s) + 2H+ (aq) → H2O (l) + CO2 (g) + Ni2+ (aq)
D) NiCO3 (s) + 2HI (aq) → 2 H2O (l) + CO2 (g) + NiI2 (aq)
E) NiCO3 (s) + 2HI (aq) → H2O (l) + CO2 (g) + Ni2+ (aq) + 2 I- (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) → 3 H2O (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) → 3 H2O (l) + Al3+ (aq)
E) Al(OH)3 (s) + 3HNO3 (aq) → 3 H2O (l) + Al3+ (aq) + NO3- (aq)
7) Which of the following is soluble in water at 25 °C?
A) Fe3 (PO4)2
B) Fe(OH)2
C) Fe(NO3)2
D) FeCO3
E) FeS
8) 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
9) 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
10) Which one of the following compounds is insoluble in water?
A) Na2CO3
B) K2SO4
C) Fe(NO3)3
D) ZnS
E) AgNO3
11) Which one of the following compounds is insoluble in water?
A) K2SO4
B) Ca(C2H3O2)2
C) MgC2O4
D) ZnCl2
E) Mn(NO3)2
12) 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) NaOH (aq) and HCl (aq)
13) 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 H C2H3O2 (aq)
E) NaOH (aq) and Fe(NO3)2 (aq)
14) 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)
15) 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
16) With which of the following will the potassium ion form an insoluble salt?
A) chloride
B) sulfate
C) carbonate
D) sulfate and carbonate
E) none of the above
17) The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide is __________.
A) H+ (aq) + HSO4- (aq) + 2OH- (aq) → 2 H2O (l) + SO42- (aq)
B) H+ (aq) + HSO4- (aq) + 2 Na+ (aq) + 2OH- (aq) → 2 H2O (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) → 2 H2O (l) + 2Na+ (aq) + SO42- (aq)
18) The net ionic equation for the reaction between aqueous nitric acid and aqueous sodium hydroxide is __________.
A) H+ (aq) + HNO3 (aq) + 2OH- (aq) → 2 H2O (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)
19) 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
20) Which one of the following is a diprotic acid?
A) nitric acid
B) chloric acid
C) phosphoric acid
D) hydrofluoric acid
E) sulfuric acid
21) Which one of the following is a triprotic acid?
A) nitric acid
B) chloric acid
C) phosphoric acid
D) hydrofluoric acid
E) sulfuric acid
22) Which one of the following solutions will have the greatest concentration of hydroxide ions?
A) 0.300 M rubidium hydroxide
B) 0.100 M magnesium hydroxide
C) 0.100 M ammonia
D) 0.100 M beryllium hydroxide
E) 0.100 M hydrochloric acid
23) Which one of the following is a weak acid?
A) HNO3
B) HCl
C) HI
D) HF
E) HClO4
24) Which of the following are weak acids?
A) HF, HBr
B) HI, HNO3, HBr
C) HI, HF
D) HF
E) none of the above
25) 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+
26) Which hydroxides are weak bases?
A) KOH, Ba(OH)2
B) Sr(OH)2, KOH, NaOH, Ba(OH)2
C) KOH, NaOH
D) KOH, NaOH, Ba(OH)2
E) None of these is a weak base.
27) The balanced reaction between aqueous potassium hydroxide and aqueous acetic acid is __________.
A) KOH (aq) + HC2H3O2 (aq) → OH- (l) + H C2H3O2+ (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)
28) 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) → 2 H2O (l) + Sr(NO3)2 (aq)
E) 2HNO3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + 2 H2 (g)
29) In which reaction does the oxidation number of oxygen increase?
A) Ba(NO3)2 (aq) + K2SO4 (aq) → BaSO4 (s) + 2 KNO3 (aq)
B) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
C) MgO (s) + H2O (l) → Mg(OH)2 (s)
D) 2 SO2 (g) + O2 (g) → 2 SO3 (g)
E) 2 H2O (l) → 2 H2 (g) + O2 (g)
30) In which reaction does the oxidation number of hydrogen change?
A) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
B) 2 Na (s) + 2 H2O (l) → 2 NaOH (aq) + H2 (g)
C) CaO (s) + H2O (l) → Ca(OH)2 (s)
D) 2 HClO4 (aq) + CaCO3 (s) → Ca(ClO4)2 (aq) + H2O (l) + CO2 (g)
E) SO2 (g) + H2O (l) → H2SO3 (aq)
31) In which species does sulfur have the highest oxidation number?
A) S8 (elemental form of sulfur)
B) H2S
C) SO2
D) H2SO3
E) K2SO4
32) In which species does nitrogen have the highest oxidation number?
A) N2
B) NH3
C) HNO2
D) NO2-
E) NaNO3
33) Which compound has the atom with the highest oxidation number?
A) CaS
B) Na3N
C) MgSO3
D) Al(NO2)3
E) NH4Cl
34) 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
35) Which of these metals will be oxidized by the ions of cobalt?
A) nickel
B) tin
C) iron
D) copper
E) silver
36) Which of these metals will be oxidized by the ions of aluminum?
A) magnesium
B) zinc
C) chromium
D) iron
E) nickel
37) 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
38) 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) + 3 H2 (g)
E) Zn (s) + 2HI (aq) → ZnI2 (aq) + H2 (g)
39) 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)
40) 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.
41) 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)
42) 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+
43) 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
44) 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
45) Oxidation and __________ mean essentially the same thing.
A) activity
B) reduction
C) metathesis
D) decomposition
E) corrosion
46) Oxidation cannot occur without __________.
A) acid
B) oxygen
C) water
D) air
E) reduction
47) 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)
48) 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)
49) 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
50) 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 6.67 × 10-2 mol of Ca2+.
51) 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
52) Which solution has the same number of moles of NaOH as 50.00 mL of 0.100M solution of NaOH?
A) 20.00 mL of 0.200M solution of NaOH
B) 25.00 mL of 0.175M solution of NaOH
C) 30.00 mL of 0.145M solution of NaOH
D) 50.00 mL of 0.125M solution of NaOH
E) 100.00 mL of 0.0500M solution of NaOH
53) Which solution has the same number of moles of KCl as 75.00 mL of 0.250M solution of KCl?
A) 20.0 mL of 0.200M solution of KCl
B) 25.0 mL of 0.175M solution of KCl
C) 129 mL of 0.145M solution of KCl
D) 50.0 mL of 0.125M solution of KCl
E) 100 mL of 0.0500M solution of KCl
54) 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
55) What are the respective concentrations (M) of Mg+2 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
56) What are the respective concentrations (M) of Cu+2 and Cl- afforded by dissolving 0.200 mol CuCl2 in water and diluting to 345 mL?
A) 0.200 and 0.200
B) 0.580 and 1.16
C) 0.200 and 0.400
D) 1.16 and 2.32
E) 0.580 and 0.290
57) 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
58) 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
59) 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.
60) 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
61) Which solution contains the largest number of moles of chloride ions?
A) 10.0 mL of 0.500M BaCl2
B) 4.00 mL of 1.000M NaCl
C) 7.50 mL of 0.500M FeCl3
D) 25.00 mL of 0.400M KCl
E) 30.00 mL of 0.100M CaCl2
62) What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200. mL to make a 1.50 M solution of sodium hydroxide?
A) 0.0500
B) 50.0
C) 45.0
D) 800.
E) 0.800
63) 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
64) 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
65) 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
66) What volume (ml) of a 3.45 M lead nitrate solution must be diluted to 450.0 ml to make a 0.990 M solution of lead nitrate?
A) 129
B) 109
C) 101
D) 56
E) 45
67) What mass (g) of barium iodide is contained in 250 mL of a barium iodide solution that has an iodide ion concentration of 0.193 M?
A) 9.44
B) 18.9
C) 0.024
D) 0.048
E) 37.7
68) What mass (g) of AgBr is formed when 35.5 mL of 0.184 M AgNO3 is treated with an excess of aqueous hydrobromic acid?
A) 1.44
B) 1.23
C) 53.6
D) 34.5
E) 188
69) What mass (g) of CaF2 is formed when 47.8 mL of 0.334 M NaF is treated with an excess of aqueous calcium nitrate?
A) 1.25
B) 0.472
C) 2.49
D) 0.943
E) 0.623
70) What volume (mL) of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129 M HCl?
A) 13.1
B) 0.24
C) 14.3
D) 0.076
E) 6.55
71) 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 × 
72) 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
73) The point in a titration at which the indicator changes is called the __________.
A) setpoint
B) indicator point
C) standard point
D) endpoint
E) volumetric point
74) 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
75) 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
76) A 36.3 mL aliquot of 0.0529 M H2SO4 (aq) is to be titrated with 0.0411 M NaOH (aq). What volume (mL) of base will it take to reach the equivalence point?
A) 93.4
B) 46.7
C) 187
D) 1.92
E) 3.84
77) A 13.8 mL aliquot of 0.176 M H3PO4 (aq) is to be titrated with 0.110 M NaOH (aq). What volume (mL) of base will it take to reach the equivalence point?
A) 7.29
B) 22.1
C) 199
D) 66.2
E) 20.9
78) 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
79) What volume (mL) of 7.48 × 10-2 M phosphoric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide?
A) 125
B) 375
C) 750
D) 188
E) 75.0
80) __________ 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
HC2H3O2NH3
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?
HCl
HC2H3O2
NH3
KCl
A) HCl, KCl
B) HCl, HC2H3O2, NH3, KCl
C) HC2H3O2, KCl
D) HC2H3O2, NH3
E) HCl, HC2H3O2, KCl
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 ion(s) is/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 ion(s) is/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) Ca2+ (aq) + CO32- (aq) → CaCO3 (s)
E) Na2CO3 (aq) + CaCl2 (aq) → 2NaCl (aq) + CaCO3 (s)
12) When aqueous solutions of AgN O3 and KI are mixed, AgI precipitates. The balanced net ionic equation is __________.
A) Ag+ (aq) + I- (aq) → AgI (s)
B) Ag+ (aq) + NO3- (aq) → AgNO3 (s)
C) Ag+ (aq) + NO3- (aq) → AgNO3 (aq)
D) AgNO3 (aq) + KI (aq) → AgI (s) + KNO3 (aq)
E) AgNO3 (aq) + KI (aq) → AgI (aq) + KNO3 (s)
13) When aqueous solutions of AgNO3 and NaCl are mixed, AgCl precipitates. The balanced net ionic equation is __________.
A) Ag+ (aq) + Cl- (aq) → AgCl (s)
B) Ag+ (aq) + NO3- (aq) → AgNO3 (s)
C) Ag+ (aq) + NO3- (aq) → AgNO (aq)
D) AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq)
E) AgNO3 (aq) + NaCl (aq) → AgCl (aq) + NaNO3 (s)
14) When H2SO4 is neutralized by NaOH in aqueous solution, the net ionic equation is __________.
A) SO42- (aq) + 2Na+ (aq) → Na2SO4 (aq)
B) SO42- (aq) + 2Na+ (aq) → Na2SO4 (s)
C) H+ (aq) + OH- (aq) → H2O (l)
D) H2SO4 (aq) + 2OH- (aq) → 2 H2O (l) + SO42- (aq)
E) 2H+ (aq) + 2NaOH (aq) → 2 H2O (l) + 2Na+ (aq)
15) The spectator ions in the reaction between aqueous perchloric acid and aqueous barium hydroxide are __________.
A) OH- and ClO4-
B) H+, OH-, ClO4-, and Ba2+
C) H+ and OH-
D) H+ and Ba2+
E) ClO4- and Ba2+
16) The spectator ions in the reaction between aqueous chloric acid and aqueous barium hydroxide are __________.
A) OH- and ClO3-
B) H+, OH-, ClO3-, and Ba2+
C) H+ and OH-
D) H+ and Ba2+
E) ClO3- and Ba2+
17) The spectator ions in the reaction between aqueous hydrofluoric acid and aqueous barium hydroxide are __________.
A) OH-, F-, and Ba2+
B) F- and Ba2+
C) OH- and F-
D) Ba2+ only
E) H+, OH-, F-, and Ba2+
18) The spectator ions in the reaction between aqueous hydrochloric acid and aqueous ammonia are __________.
A) H+ and NH3
B) H+, Cl-, NH3, and NH4+
C) Cl- and NH4+
D) H+, Cl-, and NH4+
E) Cl- only
19) Which of the following are strong acids?
HI
HNO3
HF
HBr
A) HF, HBr
B) HI, HNO3, HF, HBr
C) HI, HF, HBr
D) HNO3, HF, HBr
E) HI, HNO3, HBr
20) Which hydroxides are strong bases?
Sr (OH)2
KOH
NaOH
Ba(OH)2
A) KOH, Ba(OH)2
B) KOH, NaOH
C) KOH, NaOH, Ba(OH)2
D) Sr)OH)2, KOH, NaOH, Ba(OH)2
E) None of these is a strong base.
21) A neutralization reaction between an acid and a metal hydroxide produces __________.
A) water and a salt
B) hydrogen gas
C) oxygen gas
D) sodium hydroxide
E) ammonia
22) Of the metals below, only __________ will not dissolve in an aqueous solution containing nickel ions.
aluminum
chromium
barium
tin
potassium
A) aluminum
B) chromium
C) barium
D) tin
E) potassium
23) Which of these metals is the least easily oxidized?
Na
Au
Fe
Ca
Ag
A) Na
B) Au
C) Fe
D) Ca
E) Ag
24) Which of these metals is the most easily oxidized?
Na
Au
Fe
Ca
Ag
A) Na
B) Au
C) Fe
D) Ca
E) Ag
25) Of the following elements, __________ is the only one that cannot be found in nature in its elemental form.
Cu
Hg
Au
Ag
Na
A) Cu
B) Hg
C) Au
D) Ag
E) Na
26) Of the following elements, __________ is the most easily oxidized.
oxygen
fluorine
nitrogen
aluminum
gold
A) oxygen
B) fluorine
C) nitrogen
D) aluminum
E) gold
27) Of the following elements, __________ is the least easily oxidized.
zinc
iron
hydrogen
aluminum
lead
A) zinc
B) iron
C) hydrogen
D) aluminum
E) lead
28) Based on the equations below, which metal is the most active?
Pb(NO3)2 (aq) + Ni (s) → Ni(NO3)2 (aq) + Pb (s)
Pb(NO3)2 (aq) + Ag (s) → No reaction
Cu(NO3)2 (aq) + Ni (s) → Ni(NO3)2 (aq) + Cu (s)
A) Ni
B) Ag
C) Cu
D) Pb
E) N
29) When gold dissolves in aqua regia, what is reduced?
A) H+
B) N+5
C) Cl-
D) H2O
E) Au
30) What is the concentration (M) of a NaCl solution prepared by dissolving 9.3 g of NaCl in sufficient water to give 350 mL of solution?
A) 18
B) 0.16
C) 0.45
D) 27
E) 2.7 × 10-2
31) How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2?
A) 2.00
B) 0.500
C) 0.160
D) 0.0800
E) 0.0400
32) How many moles of Na+ are present in 343 mL of a 1.27 M solution of Na2SO4?
A) 0.436
B) 0.871
C) 1.31
D) 3.70
E) 11.1
33) How many moles of K+ are present in 343 mL of a 1.27 M solution of K3PO4?
A) 0.436
B) 1.31
C) 0.145
D) 3.70
E) 11.1
34) What are the respective concentrations (M) of Na+ and SO42- afforded by dissolving 0.500 mol Na2SO4 in water and diluting to 1.33 L?
A) 0.665 and 0.665
B) 0.665 and 1.33
C) 1.33 and 0.665
D) 0.376 and 0.752
E) 0.752 and 0.376
35) What are the respective concentrations (M) of K+ and PO43- afforded by dissolving 0.800 mol K3PO4 in water and diluting to 1.63 L?
A) 0.800 and 0.800
B) 0.491 and 0.491
C) 0.800 and 0.491
D) 1.44 and 0.491
E) 0.489 and 0.163
36) Calculate the concentration (M) of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M solution of sodium sulfide to a total volume of 250.0 mL.
A) 0.175
B) 4.37
C) 0.525
D) 0.350
E) 0.874
37) An aqueous ethanol solution (400 mL) was diluted to 4.00 L, giving a concentration of 0.0400 M. The concentration of the original solution was __________ M.
A) 0.400
B) 0.200
C) 2.00
D) 1.60
E) 4.00
38) The concentration (M) of an aqueous methanol produced when 0.200 L of a 2.00 M solution was diluted to 0.800 L is __________.
A) 0.800
B) 0.200
C) 0.500
D) 0.400
E) 8.00
39) The molarity (M) of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of solution is __________.
A) 0.0657
B) 1.85 × ![clip_image002[1]](https://www.coursepaper.com/wp-content/uploads/2014/03/clip_image002123.jpg "clip_image002[1]"){kind=small}
C) 1.85
D) 3.52
E) 0.104
40) The molarity (M) of an aqueous solution containing 52.5 g of sucrose (C12H22O11) in 35.5 mL of solution is __________.
A) 5.46
B) 1.48
C) 0.104
D) 4.32
E) 1.85
41) The molarity (M) of an aqueous solution containing 22.5 g of glucose (C6H12O6) in 35.5 mL of solution is __________.
A) 3.52
B) 0.634
C) 0.197
D) 0.125
E) 1.85
42) The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6) in 35.5 mL of solution is __________.
A) 1.85
B) 2.12
C) 0.197
D) 3.52
E) 11.8
43) How many grams of sodium chloride are there in 55.0 mL of a 1.90 M aqueous solution of sodium chloride?
A) 0.105
B) 6.11
C) 3.21
D) 6.11 × 103
E) 12.2
44) How many grams of sodium chloride are there in 550.0 mL of a 1.90 M aqueous solution of sodium chloride?
A) 61.1
B) 1.05
C) 30.5
D) 6.11 × 104
E) 122
45) The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500. mL is __________.
A) 0.0879
B) 87.9
C) 0.0218
D) 0.0115
E) 0.870
46) The molarity of a solution prepared by diluting 43.72 mL of 5.005 M aqueous K2Cr2O7 to 500. mL is __________.
A) 57.2
B) 0.0044
C) 0.438
D) 0.0879
E) 0.870
47) The concentration of chloride ions in a 0.193 M solution of potassium chloride is __________.
A) 0.0643 M
B) 0.386 M
C) 0.0965 M
D) 0.579 M
E) 0.193 M
48) The concentration of sulfate ions in a 0.233 M solution of sulfuric acid is __________.
A) 0.699 M
B) 0.233 M
C) 0.466 M
D) 0.0777 M
E) 0.155 M
49) The concentration of iodide ions in a 0.193 M solution of barium iodide is __________.
A) 0.193 M
B) 0.386 M
C) 0.0965 M
D) 0.579 M
E) 0.0643 M
50) The concentration of species in 500 mL of a 2.104 M solution of sodium sulfate is __________ M sodium ion and __________ M sulfate ion.
A) 2.104, 1.052
B) 2.104, 2.104
C) 2.104, 4.208
D) 1.052, 1.052
E) 4.208, 2.104
51) When 0.500 mol of HC2H3O2 is combined with enough water to make a 300.0 mL solution, the concentration of HC2H3O2 is __________ M.
A) 3.33
B) 1.67
C) 0.835
D) 0.00167
E) 0.150
52) In a titration of 35.00 mL of 0.737 M H2SO4, __________ mL of a 0.827 M KOH solution is required for neutralization.
A) 35.0
B) 1.12
C) 25.8
D) 62.4
E) 39.3
53) Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H2C2O4) in a solid given that a 0.7984-g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization.
A) 48.89
B) 97.78
C) 28.59
D) 1.086
E) 22.83
54) Oxalic acid is a diprotic acid. If a solid material contains 53.66 percent of oxalic acid (H2C2O4), by mass, then a 0.6543-g sample of that solid will require __________ mL of 0.3483 M NaOH for neutralization.
A) 11.19
B) 97.78
C) 28.59
D) 1.119
E) 22.39
55) A 17.5 mL sample of an acetic acid (CH3CO2H) solution required 29.6 mL of 0.250 M NaOH for neutralization. The concentration of acetic acid was __________ M.
A) 0.158
B) 0.423
C) 134
D) 6.88
E) 0.214
56) A 25.5 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.113 M NaOH (aq). It took 51.2 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was __________.
A) 1.02
B) 0.114
C) 0.454
D) 0.113
E) 0.227
57) A 31.5 mL aliquot of HNO3 (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was __________.
A) 0.0102
B) 0.0051
C) 0.0204
D) 0.227
E) 1.02
58) A 31.5 mL aliquot of H2SO4 (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was __________.
A) 0.0102
B) 0.00508
C) 0.0204
D) 0.102
E) 0.227
4.3 Algorithmic Questions
1) The total concentration of ions in a 0.625 M solution of HCl is __________.
A) 0
B) 0.500 M
C) 0.625 M
D) 1.25 M
E) 1.50 M
2) What is the concentration (M) of sodium ions in 4.57 L of a 1.25 M Na3PO4 solution?
3) How many grams of NaOH (MW = 40.0) are there in 500.0 mL of a 0.225 M NaOH solution?
A) 0.00219
B) 114
C) 14.0
D) 4.50
E) 0.113
4) How many grams of NaOH (MW = 40.0) are there in 100.0 mL of a 0.175 M NaOH solution?
A) .00219
B) 114
C) 0.700
D) 0.0175
E) 14.0
5) How many grams of CH3OH must be added to water to prepare 150 mL of a solution that is 1.0 M CH3OH?
A) 0.15
B) 430
C) 2.4
D) 4.8
E) 4.3
6) There are __________ mol of bromide ions in 0.500 L of a 0.100 M solution of AlBr3.
A) 0.0500
B) 0.450
C) 0.150
D) 0.167
E) 0.500
7) What is the concentration (M) of KCl in a solution made by mixing 30.0 mL of 0.100 M KCl with 50.0 mL of 0.100 M KCl?
A) 0.100
B) 0.0500
C) 0.0333
D) 0.0250
E) 125
8) What is the concentration (M) of CH3OH in a solution prepared by dissolving 29.3 g of CH3OH in sufficient water to give exactly 230 mL of solution?
A) 11.9
B) 0.00159
C) 1.59
D) 3.97
E) 4.31
9) What is the concentration (M) of CH3OH in a solution prepared by dissolving 11.7 g of CH3OH in sufficient water to give exactly 230. mL of solution?
A) 11.9
B) 1.59
C) 0.00159
D) 3.17
E) 0.0841
10) How many grams of H3PO4 are in 175 mL of a 3.50 M solution of H3PO4?
A) 0.610
B) 60.0
C) 20.0
D) 4.90
E) 612
11) How many grams of H3PO4 are in 175 mL of a 2.50 M solution of H3PO4?
A) 0.438
B) 20.0
C) 42.9
D) 4.90
E) 612
12) What is the concentration (M) of CH3OH in a solution prepared by dissolving 16.8 g of CH3OH in sufficient water to give exactly 230 mL of solution?
13) How many grams of H3PO4 are in 265 mL of a 1.50 M solution of H3PO4?
14) What is the concentration (M) of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?
15) How many grams of NaOH (MW = 40.0) are there in 250.0 mL of a 0.275 M NaOH solution?
16) How many grams of CH3OH must be added to water to prepare 150mL of a solution that is 2.0 M CH3OH?
17) There are __________ mol of bromide ions in 0.900 L of a 0.500M solution of AlBr3.
18) How many moles of Co2+ are present in 0.150 L of a 0.200 M solution of CoI2?
19) Calculate the concentration (M) of sodium ions in a solution made by diluting 40.0 mL of a 0.474 M solution of sodium sulfide to a total volume of 300 mL.
20) How many milliliters of a stock solution of 11.1 M HNO3 would be needed to prepare 0.500 L of 0.500 M HNO3?
A) 0.0444
B) 22.5
C) 2.78
D) 44.4
E) 0.0225
21) A stock solution of HNO3 is prepared and found to contain 13.5 M of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is __________ M.
A) 0.270
B) 1.48
C) 0.675
D) 675
E) 270
22) Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 10.00 mL of glacial acetic acid at 25 °C in sufficient water to give 500.0 mL of solution. The density of glacial acetic acid at 25 °C is 1.05 g/mL.
A) 1.26 × 103
B) 21.0
C) 0.0210
D) 0.350
E) 3.50 × 10-4
23) A solution is prepared by mixing 50.0 mL of 0.100 M HCl and 10.0 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution?
A) 0.183
B) 8.57
C) 3.50
D) 0.0500
E) 0.117
24) A solution is prepared by adding 1.60 g of solid NaCl to 50.0 mL of 0.100 M CaCl2. What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.
A) 0.747
B) 0.647
C) 0.132
D) 0.232
E) 0.547
25) Calculate the number of grams of solute in 500.0 mL of 0.189 M KOH.
A) 148
B) 1.68
C) 5.30 × 103
D) 5.30
E) 1.68 × 10-3
26) What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution?
A) 0.801
B) 0.315
C) 0.629
D) 125
E) 0.400
27) Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide:
Pb2+ (aq) + 2I- (aq) → PbI2 (s)
Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 0.700 mol of Pb(NO)3)2 (aq) to completely precipitate the lead?
A) 2.54 × 10-3
B) 394
C) 197
D) 0.197
E) 0.394
28) Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride:
Ag+ (aq) + Cl- (aq) → AgCl (s)
Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.366 M AgNO3 solution to completely precipitate the silver?
A) 9.15 × 10-3
B) 1.57 × 10-4
C) 0.535
D) 0.157
E) 6.39 × 103
29) How many milliliters of 0.132 M HClO4 solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?
A) 0.521
B) 0.0120
C) 83.7
D) 0.0335
E) 29.9
4.4 Short Answer Questions
1) The solvent in an aqueous solution is __________.
2) What is aqua regia?
3) When gold dissolves in aqua regia, into what form is the gold converted?
4) Calculate the concentration (M) of arsenic acid (H3AsO4) in a solution if 25.00 mL of that solution required 35.21 mL of 0.1894 M KOH for neutralization.
5) How many moles of BaCl2 are formed in the neutralization of 393 mL of 0.171 M Ba(OH)2 with aqueous HCl?
4.5 True/False Questions
1) Ca(OH)2 is a strong base.
2) The compound HClO4 is a weak acid.
3) HNO2 is a strong acid.
4) The compound NH4Cl is a weak acid.
5) Ammonia is a strong base.
Answer:
View Answer