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Practice problems and practice test for exam 2
chapter 4 and chapter 10
Chapter 4 Reactions in Aqueous Solution
1) Of the species below, only __________ is not an electrolyte.
A) HCl
B) Rb2SO4
C) Ar
D) KOH
E) NaCl
2) 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
3) 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)
4) 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)
5) 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
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6) 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
7) 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
8) Which one of the following compounds is insoluble in water?
A) Na2CO3
B) K2SO4
C) Fe(NO3)3
D) ZnS
E) AgNO3
9) Which one of the following compounds is insoluble in water?
A) K2SO4
B) Ca(C2H3O2)2
C) MgC2O4
D) ZnCl2
E) Mn(NO3)2
10) 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)
11) 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)
12) Which combination will produce a precipitate?
A) Pb(NO3)2 (aq) and HCl (aq)
B) Cu(NO3)2 (aq) and KC2H3O2 (aq)
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C) KOH (aq) and HNO3 (aq)
D) AgC2H3O2 (aq) and HC2H3O2 (aq)
E) NaOH (aq) and Sr(NO3)2 (aq)
13) 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)
14) 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)
15) Which one of the following is a diprotic acid?
A) nitric acid
B) chloric acid
C) phosphoric acid
D) hydrofluoric acid
E) sulfuric acid
16) Which one of the following is a triprotic acid?
A) nitric acid
B) chloric acid
C) phosphoric acid
D) hydrofluoric acid
E) sulfuric acid
17) Which one of the following is a weak acid?
A) HNO3
B) HCl
C) HI
D) HF
E) HClO4
18) Which of the following are weak acids?
A) HF, HBr
B) HI, HNO3, HBr
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C) HI, HF
D) HF
E) none of the above
19) 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.
20) 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)
21) 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)
22) In which species does nitrogen have the highest oxidation number?
A) N2
B) NH3
C) HNO2
D) NO2E) NaNO3
23) Which compound has the atom with the highest oxidation number?
A) CaS
B) Na3N
C) MgSO3
D) Al(NO2)3
E) NH4Cl
24) 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)
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E) Zn (s) + 2HI (aq) → ZnI2 (aq) + H2 (g)
25) 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)
26) Oxidation and __________ mean essentially the same thing.
A) activity
B) reduction
C) metathesis
D) decomposition
E) corrosion
27) Oxidation cannot occur without __________.
A) acid
B) oxygen
C) water
D) air
E) reduction
28) 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)
29) 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
30) 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
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31) 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
32) 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
33) 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
34) 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
35) 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
36) 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
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37) A strong electrolyte is one that __________ completely in solution.
A) reacts
B) associates
C) disappears
D) ionizes
38) 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
39) 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
40) 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
41) Which hydroxides are strong bases?
Sr (OH)2
KOH
NaOH
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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.
42) 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.40) The molarity (M) of an aqueous solution
containing 52.5 g of sucrose (C12H22O11) in 35.5 mL of solution is __________.
43) The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500. mL is
__________.
44) The concentration of chloride ions in a 0.193 M solution of potassium chloride is __________.
45) How many grams of H3PO4 are in 265 mL of a 1.50 M solution of H3PO4?
46) 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.
Chapter 10 Gases
1) Which of the following statements about gases is false?
A) Gases are highly compressible.
B) Distances between molecules of gas are very large compared to bond distances within molecules.
C) Non-reacting gas mixtures are homogeneous.
D) Gases expand spontaneously to fill the container they are placed in.
E) All gases are colorless and odorless at room temperature.
2) Gaseous mixtures __________.
A) can only contain molecules
B) are all heterogeneous
C) can only contain isolated atoms
D) are all homogeneous
E) must contain both isolated atoms and molecules
3) Of the following, __________ is a correct statement of Boyle's law.
A) PV = constant
P
B)
= constant
V
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V
= constant
P
V
D)
= constant
T
n
E)
= constant
P
C)
4) Of the following, __________ is a valid statement of Charles' law.
P
A)
= constant
T
V
B)
= constant
T
C) PV = constant
D) V = constant × n
E) V = constant × P
5) Which one of the following is a valid statement of Avogadro's law?
P
A)
= constant
T
V
B)
= constant
T
C) PV = constant
D) V = constant × n
E) V = constant × P
6) The volume of an ideal gas is zero at __________.
A) 0 °C
B) -45 °F
C) -273 K
D) -363 K
E) -273 °C
7) The molar volume of a gas at STP is __________ L.
A) 0.08206
B) 62.36
C) 1.00
D) 22.4
E) 14.7
8) How many moles of gas are there in a 45.0 L container at 25.0°C and 500.0 mm Hg?
A) 0.630
B) 6.11
C) 18.4
D) 1.21
E) 207
9) How many moles of gas are there in a 50.0 L container at 22.0°C and 825 torr?
A) 2.29 × 104
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B) 1.70 × 103
C) 2.23
D) 0.603
E) 18.4
10) Standard temperature and pressure (STP), in the context of gases, refers to __________.
11) The volume of 1.20 mol of gas at 61.3 kPa and 25.0°C is __________ L.
12) The density of NO2 in a 3.50 L tank at 780.0 torr and 37.0°C is __________ g/L.
A) 1.64
B) 9.30
C) 1.86
D) 2.92
E) 3.27
13) A mixture of Xe, Kr, and Ar has a total pressure of 6.70 atm. What is the mole fraction of Kr if the partial
pressures of Xe and Ar are 1.60 atm and 2.80 atm, respectively.
A) 0.174
B) 0.256
C) 0.343
D) 0.481
E) 0.570
14) A gas at a pressure of 10.0 Pa exerts a force of __________ N on an area of 5.5 m2.
A) 55
B) 0.55
C) 5.5
D) 1.8
E) 18
15) If 50.75 g of a gas occupies 10.0 L at STP, 129.3 g of the gas will occupy __________ L at STP.
16) A sample of H2 gas (12.28 g) occupies 100.0 L at 400.0 K and 2.00 atm. A sample weighing 9.49 g
occupies __________ L at 353 K and 2.00 atm.
17) The amount of gas that occupies 60.82 L at 31.0°C and 367 mm Hg is __________ mol.
A) 1.18
B) 0.850
C) 894
D) 11.6
E) 0.120
18) The temperature of a sample of CH4 gas (10.34 g) in a 50.0 L vessel at 1.33 atm is __________ °C.
A) 984
B) -195
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C) 195
D) 1260
E) -1260
19) The density of ammonia gas in a 4.32 L container at 837 torr and 45.0°C is __________ g/L.
20) A vessel contained N2, Ar, He, and Ne. The total pressure in the vessel was 987 torr. The partial pressures
of nitrogen, argon, and helium were 44.0, 486, and 218 torr, respectively. The partial pressure of neon in the
vessel was __________ torr.
A) 42.4
B) 521
C) 19.4
D) 239
E) 760
21) A pressure of 1.25 atm is the same as a pressure of __________ of mm Hg.
A) 193
B) 760.
C) 950.
D) 29.9
E) 33.0
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