CHE 1401 - Spring 2015 - Chapter 4
Homework 4 (Chapter 4: Aqueous reactions and solution stoichimetry)
_______________________________________________________________________________
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the
question.
1) The balanced molecular equation for complete neutralization of H2SO4 by
KOH in aqueous solution is __________.
A) 2H+ (aq) + 2OH- (aq) → 2H2O (l)
B) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq)
C) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (s)
D) 2H+ (aq) + 2KOH (aq) → 2H2O (l) + 2K+ (aq)
E) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq)
1)
2) 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) 800.
B) 45.0
C) 0.0500
D) 50.0
E) 0.800
2)
3) 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) 75.0
C) 188
D) 750
E) 375
3)
4) In which reaction does the oxidation number of hydrogen change?
A) CaO (s) + H2O (l) → Ca(OH)2 (s)
4)
B) 2 HClO4 (aq) + CaCO3 (s) → Ca(ClO4)2 (aq) + H2O (l) + CO2 (g)
C) 2 Na (s) + 2 H2O (l) → 2 NaOH (aq) + H2 (g)
D) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
E) SO2(g) + H2O (l) → H2SO3 (aq)
5) 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) 1.92
D) 93.4
E) 3.84
5)
6) 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) 0.623
B) 0.943
C) 0.472
D) 2.49
E) 1.25
6)
1
7) Which combination will produce a precipitate?
A) NaC2H3O2 (aq) and HCl (aq)
B) NaOH (aq) and HCl (aq)
C) AgNO 3 (aq) and Ca(C2H3O 2)2 (aq)
D) NaOH (aq) and HCl (aq)
E) KOH (aq) and Mg(NO 3)2 (aq)
8) Which of these metals will be oxidized by the ions of cobalt?
A) iron
B) copper
C) nickel
D) silver
7)
8)
E) tin
9) Which one of the following is a correct expression for molarity?
A) mol solute/L solvent
B) μmol solute/L solution
C) mol solute/kg solvent
D) mmol solute/mL solution
E) mol solute/mL solvent
9)
10) 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) 0.414
B) 7.28
C) 1.64
D) 0.173
E) 0.207
10)
11) When aqueous solutions of __________ are mixed, a precipitate forms.
A) K2SO4 and CrCl3
B) NaI and KBr
C) NiBr2 and AgNO3
D) Li2CO3 and CsI
E) KOH and Ba(NO3)2
11)
12) 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) 0.675
B) 0.270
C) 675
D) 1.48
E) 270
12)
13) __________ is an oxidation reaction.
A) Table salt dissolving in water for cooking vegetables
B) Rusting of iron
C) Ice melting in a soft drink
D) Neutralization of HCl by NaOH
E) The reaction of sodium chloride with lead nitrate to form lead chloride
and sodium nitrate
13)
2
14) 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) 50.0
B) 2.64
C) 26.4
D) 176
E) 29.3
14)
15) Which hydroxides are weak bases?
A) KOH, Ba(OH)2
B) Sr(OH)2, KOH, NaOH, Ba(OH)2
C) KOH, NaOH, Ba(OH)2
15)
D) KOH, NaOH
E) None of these is a weak base.
16) Based on the activity series, which one of the reactions below will occur?
A) Mn (s) + NiCl2 (aq) → MnCl2 (aq) + Ni (s)
B) SnBr2 (aq) + Cu (s) → CuBr2 (aq) + Sn (s)
C) Pb (s) + NiI2 (aq) → PbI2 (aq) + Ni (s)
D) Fe (s) + ZnCl2 (aq) → FeCl2 (aq) + Zn (s)
E) None of the reactions will occur.
16)
17) Oxidation and __________ mean essentially the same thing.
A) decomposition
B) reduction
C) activity
D) metathesis
E) corrosion
17)
18) 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) AgNO3
B) KBr
C) Pb(NO3)2
D) Li2CO3
E) (NH4)2S
18)
3
19) 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) Fe < Ni < Co < Al < Zn
B) Zn < Al < Co < Ni < Fe
C) Ni < Co < Fe < Zn < Al
D) Ni < Fe < Co < Zn < Al
E) Co < Ni < Fe < Zn < Al
19)
20) With which of the following will the potassium ion form an insoluble salt?
A) sulfate
B) chloride
C) sulfate and carbonate
D) carbonate
E) none of the above
20)
21) 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) cobalt
C) lead
D) zinc
E) none of these
21)
22) Which one of the following is a weak acid?
A) HNO 3
B) HCl
C) HClO 4
22)
D) HF
E) HI
23) What volume (mL) of 7.48 × 10-2 M perchloric acid can be neutralized with 115
mL of 0.244 M sodium hydroxide?
A) 750
B) 188
C) 8.60
D) 375
E) 125
23)
24) 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) 0.386
B) 0.0643
C) 12.37
D) 6.19
E) 0.0830
24)
25) What volume (mL) of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129
M HCl?
A) 6.55
B) 0.24
C) 14.3
D) 0.076
E) 13.1
25)
4
26) 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 perchloric acid
B) 10.0 mL of 0.0500 M phosphoric acid
C) 15.0 mL of 0.0500 M hydrobromic acid
D) 20.0 mL of 0.0500 M nitric acid
E) 5.0 mL of 0.0100 M sulfuric acid
26)
27) 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) The product of concentration and volume of the less concentrated solution
equals the product of concentration and volume of the more concentrated
solution.
C) It would take more base solution (per milliliter of the unknown solution)
to neutralize the more concentrated solution.
D) A smaller volume of the less concentrated solution contains the same
number of moles of the acid compared to the more concentrated solution.
E) If the same volume of each sample was taken, then more base solution
would be required to neutralize the one with lower concentration.
27)
28) The point in a titration at which the indicator changes is called the __________.
A) setpoint
B) endpoint
C) indicator point
D) volumetric point
E) standard point
28)
29) Of the species below, only __________ is not an electrolyte.
A) Ar
B) KOH
C) NaCl
D) HCl
E) Rb2SO4
29)
30) Which of the following is insoluble in water at 25°C?
A) Ba(C2H3O 2)2
B) (NH4)2CO3
C) Mg3(PO4)2
D) Na2S
E) Ca(OH)2
30)
5
31) Which one of the following is a triprotic acid?
A) nitric acid
B) hydrofluoric acid
C) chloric acid
D) phosphoric acid
E) sulfuric acid
31)
32) The net ionic equation for the reaction between aqueous nitric acid and aqueous 32)
sodium hydroxide is __________.
A) H+ (aq) + Na+ (aq) +OH- (aq) → H2O (l) + Na+ (aq)
B) HNO3 (aq) + NaOH (aq) → NaNO3 (aq) + H2O (l)
C) H+ (aq) + HNO3 (aq) + 2OH- (aq) → 2H2O (l) + NO3- (aq)
D) HNO3 (aq) + OH- (aq) → NO3- (aq) + H2O (l)
E) H+ (aq) + OH- (aq) → H2O (l)
33) The balanced reaction between aqueous nitric acid and aqueous strontium
hydroxide is __________.
A) HNO 3 (aq) + Sr(OH)2 (aq) → H2O (l) + Sr(NO3)2 (aq)
B) 2HNO 3 (aq) + Sr(OH)2 (aq) → 2H2O (l) + Sr(NO3)2 (aq)
C) HNO 3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + H2 (g)
33)
D) 2HNO 3 (aq) + Sr(OH)2 (aq) → Sr(NO3)2 (aq) + 2H2 (g)
E) HNO 3 (aq) + SrOH (aq) → H2O (l) + SrNO3 (aq)
34) Based on the activity series, which one of the reactions below will occur?
A) SnCl2 (aq) + Cu (s) → Sn (s) + CuCl2 (aq)
B) 3Hg (l) + 2Cr(NO3)3 (aq) → 3Hg(NO3)2 + 2Cr (s)
C) 3FeBr2 (aq) + 2Au (s) → 3Fe (s) + 2AuBr3 (aq)
D) 2AgNO 3 (aq) + Pb (s) → 2Ag (s) + Pb(NO3)2 (aq)
34)
E) Zn (s) + MnI2 (aq) → ZnI2 (aq) + Mn (s)
35) Oxidation is the __________ and reduction is the __________.
A) gain of oxygen, loss of electrons
B) gain of electrons, loss of electrons
C) loss of electrons, gain of electrons
D) gain of oxygen, loss of mass
E) loss of oxygen, gain of electrons
6
35)
36) 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) 0.132
B) 0.747
C) 0.232
D) 0.647
E) 0.547
36)
37) Which solution contains the largest number of moles of chloride ions?
A) 10.0 mL of 0.500M BaCl2
37)
B) 30.00 mL of 0.100M CaCl2
C) 25.00 mL of 0.400M KCl
D) 4.00 mL of 1.000M NaCl
E) 7.50 mL of 0.500M FeCl3
38) Oxidation cannot occur without __________.
A) water
B) acid
C) reduction
D) oxygen
E) air
38)
39) Which of the following reactions will not occur as written?
A) Mg (s) + Ca(OH)2 (aq) → Ca (s) + Mg(OH)2 (aq)
B) Co (s) + 2AgCl (aq) → 2Ag (s) + CoCl2 (aq)
C) Co (s) + 2HI (aq) → H2 (g) + CoI2 (aq)
39)
D) Sn (s) + 2AgNO3 (aq) → 2Ag (s) + Sn(NO3)2 (aq)
E) Zn (s) + Pb(NO3)2 (aq) → Pb (s) + Zn(NO 3)2 (aq)
40) 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) 0.315
B) 0.801
C) 125
D) 0.400
E) 0.629
7
40)