CHE 1401 - Spring 2017 - Chapter 4
Homework 4 (Chapter 4: Aqueous reactions and solution stoichimetry)
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MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the
question.
1) Based on the activity series, which one of the reactions below will occur?
A) SnCl2 (aq) + Cu (s) → Sn (s) + CuCl2 (aq)
B) 2AgNO 3 (aq) + Pb (s) → 2Ag (s) + Pb(NO3)2 (aq)
1)
C) Zn (s) + MnI2 (aq) → ZnI2 (aq) + Mn (s)
D) 3Hg (l) + 2Cr(NO3)3 (aq) → 3Hg(NO3)2 + 2Cr (s)
E) 3FeBr2 (aq) + 2Au (s) → 3Fe (s) + 2AuBr3 (aq)
2) In which reaction does the oxidation number of hydrogen change?
A) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
2)
B) CaO (s) + H2O (l) → Ca(OH)2 (s)
C) SO2(g) + H2O (l) → H2SO3 (aq)
D) 2 Na (s) + 2 H2O (l) → 2 NaOH (aq) + H2 (g)
E) 2 HClO4 (aq) + CaCO3 (s) → Ca(ClO4)2 (aq) + H2O (l) + CO2 (g)
3) 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) 176
B) 29.3
C) 50.0
D) 2.64
E) 26.4
3)
4) You are given two clear solutions of the same unknown monoprotic acid, but
with different concentrations. Which statement is true?
A) A smaller volume of the less concentrated solution contains the same
number of moles of the acid compared to the more concentrated solution.
B) It would take more base solution (per milliliter of the unknown solution)
to neutralize the more concentrated solution.
C) There is no chemical method designed to tell the two solutions apart.
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.
4)
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5) The balanced reaction between aqueous nitric acid and aqueous strontium
hydroxide is __________.
A) 2HNO 3 (aq) + Sr(OH)2 (aq) → 2H2O (l) + Sr(NO3)2 (aq)
B) 2HNO 3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + 2H2 (g)
5)
C) HNO 3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + H2 (g)
D) HNO 3 (aq) + SrOH (aq) → H2O (l) + SrNO3 (aq)
E) HNO 3 (aq) + Sr(OH)2 (aq) → H2O (l) + Sr(NO3)2 (aq)
6) Which of the following would require the largest volume of 0.100 M sodium
hydroxide solution for neutralization?
A) 15.0 mL of 0.0500 M hydrobromic acid
B) 10.0 mL of 0.0500 M phosphoric acid
C) 5.0 mL of 0.0100 M sulfuric acid
D) 20.0 mL of 0.0500 M nitric acid
E) 10.0 mL of 0.0500 M perchloric acid
6)
7) 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) 0.472
B) 2.49
C) 1.25
D) 0.623
E) 0.943
7)
8) 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) 375
D) 750
E) 188
8)
9) Which of the following reactions will not occur as written?
A) Zn (s) + Pb(NO3)2 (aq) → Pb (s) + Zn(NO 3)2 (aq)
B) Co (s) + 2AgCl (aq) → 2Ag (s) + CoCl2 (aq)
C) Sn (s) + 2AgNO3 (aq) → 2Ag (s) + Sn(NO3)2 (aq)
D) Mg (s) + Ca(OH)2 (aq) → Ca (s) + Mg(OH)2 (aq)
E) Co (s) + 2HI (aq) → H2 (g) + CoI2 (aq)
9)
10) Oxidation is the __________ and reduction is the __________.
A) loss of oxygen, gain of electrons
B) loss of electrons, gain of electrons
C) gain of oxygen, loss of mass
D) gain of electrons, loss of electrons
E) gain of oxygen, loss of electrons
10)
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11) Oxidation cannot occur without __________.
A) reduction
B) oxygen
C) air
D) acid
E) water
11)
12) 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) copper
B) zinc
C) cobalt
D) lead
E) none of these
12)
13) Which of these metals will be oxidized by the ions of cobalt?
A) copper
B) iron
C) tin
D) nickel
13)
E) silver
14) Which one of the following is a triprotic acid?
A) sulfuric acid
B) hydrofluoric acid
C) nitric acid
D) chloric acid
E) phosphoric acid
14)
15) Which one of the following is a correct expression for molarity?
A) mmol solute/mL solution
B) mol solute/L solvent
C) mol solute/mL solvent
D) mol solute/kg solvent
E) μmol solute/L solution
15)
16) 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) 0.132
C) 0.232
D) 0.647
E) 0.547
16)
17) 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) 46.7
B) 187
C) 3.84
D) 93.4
E) 1.92
17)
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18) Of the species below, only __________ is not an electrolyte.
A) Rb2SO4
B) HCl
C) NaCl
D) Ar
E) KOH
18)
19) Which hydroxides are weak bases?
A) Sr(OH)2, KOH, NaOH, Ba(OH)2
19)
B) KOH, NaOH, Ba(OH)2
C) KOH, NaOH
D) KOH, Ba(OH)2
E) None of these is a weak base.
20) Which combination will produce a precipitate?
A) KOH (aq) and Mg(NO 3)2 (aq)
B) NaC2H3O2 (aq) and HCl (aq)
C) NaOH (aq) and HCl (aq)
D) AgNO 3 (aq) and Ca(C2H3O 2)2 (aq)
E) NaOH (aq) and HCl (aq)
20)
21) The net ionic equation for the reaction between aqueous nitric acid and aqueous 21)
sodium hydroxide is __________.
A) H+ (aq) + HNO3 (aq) + 2OH- (aq) → 2H2O (l) + NO3- (aq)
B) H+ (aq) + OH- (aq) → H2O (l)
C) HNO3 (aq) + NaOH (aq) → NaNO3 (aq) + H2O (l)
D) HNO3 (aq) + OH- (aq) → NO3- (aq) + H2O (l)
E) H+ (aq) + Na+ (aq) +OH- (aq) → H2O (l) + Na+ (aq)
22) Oxidation and __________ mean essentially the same thing.
A) metathesis
B) corrosion
C) activity
D) decomposition
E) reduction
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22)
23) __________ is an oxidation reaction.
A) Table salt dissolving in water for cooking vegetables
B) Rusting of iron
C) Neutralization of HCl by NaOH
D) The reaction of sodium chloride with lead nitrate to form lead chloride
and sodium nitrate
E) Ice melting in a soft drink
23)
24) Which one of the following is a weak acid?
A) HF
B) HClO4
C) HNO3
24)
D) HI
E) HCl
25) A stock solution of HNO3 is prepared and found to contain 13.5 M of HNO3. If
25)
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) 270
B) 1.48
C) 675
D) 0.270
E) 0.675
26) Based on the activity series, which one of the reactions below will occur?
A) Pb (s) + NiI2 (aq) → PbI2 (aq) + Ni (s)
B) Fe (s) + ZnCl2 (aq) → FeCl2 (aq) + Zn (s)
C) Mn (s) + NiCl2 (aq) → MnCl2 (aq) + Ni (s)
D) SnBr2 (aq) + Cu (s) → CuBr2 (aq) + Sn (s)
E) None of the reactions will occur.
26)
27) Which of the following is insoluble in water at 25°C?
A) (NH4)2CO3
B) Ba(C2H3O 2)2
C) Na2S
D) Ca(OH)2
E) Mg3(PO4)2
27)
28) 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) 50.0
B) 45.0
C) 800.
D) 0.800
E) 0.0500
28)
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29) The balanced molecular equation for complete neutralization of H2SO4 by
29)
KOH in aqueous solution is __________.
A) 2H+ (aq) + 2KOH (aq) → 2H2O (l) + 2K+ (aq)
B) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq)
C) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq)
D) 2H+ (aq) + 2OH- (aq) → 2H2O (l)
E) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (s)
30) 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) 0.414
C) 0.173
D) 0.207
E) 7.28
30)
31) Aqueous solutions of a compound did not form precipitates with Cl-, Br-, I-, S
O42-, CO32-, PO 43-, OH-, or S2-. This highly water-soluble compound
produced the foul-smelling gas H2S when the solution was acidified. This
compound is __________.
A) KBr
B) Pb(NO3)2
C) Li2CO3
D) (NH4)2S
E) AgNO3
31)
32) Which solution contains the largest number of moles of chloride ions?
A) 30.00 mL of 0.100M CaCl2
32)
B) 25.00 mL of 0.400M KCl
C) 4.00 mL of 1.000M NaCl
D) 7.50 mL of 0.500M FeCl3
E) 10.0 mL of 0.500M BaCl2
33) 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) 0.0830
B) 0.0643
C) 12.37
D) 6.19
E) 0.386
33)
34) The point in a titration at which the indicator changes is called the __________.
A) volumetric point
B) standard point
C) setpoint
D) indicator point
E) endpoint
34)
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35) What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H2SO4
35)
solution is required to neutralize a 25.0-mL sample of the NaOH solution?
A) 0.315
B) 0.801
C) 0.629
D) 0.400
E) 125
36) What volume (mL) of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129
M HCl?
A) 14.3
B) 0.24
C) 13.1
D) 6.55
E) 0.076
36)
37) With which of the following will the potassium ion form an insoluble salt?
A) sulfate
B) carbonate
C) chloride
D) sulfate and carbonate
E) none of the above
37)
38) When aqueous solutions of __________ are mixed, a precipitate forms.
A) NiBr2 and AgNO3
B) NaI and KBr
C) KOH and Ba(NO3)2
D) Li2CO3 and CsI
E) K2SO4 and CrCl3
38)
39) What volume (mL) of 7.48 × 10-2 M phosphoric acid can be neutralized with
115 mL of 0.244 M sodium hydroxide?
A) 375
B) 125
C) 750
D) 188
E) 75.0
39)
40) 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) Ni < Co < Fe < Zn < Al
B) Zn < Al < Co < Ni < Fe
C) Ni < Fe < Co < Zn < Al
D) Co < Ni < Fe < Zn < Al
E) Fe < Ni < Co < Al < Zn
40)
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