General, Organic & Biological Chemistry, 5e (Timberlake)
Chapter 9 Solutions
9.1 Multiple-Choice Questions
1) The O-H bond in water is polar because
A) it is an ionic bond.
B) oxygen is much more electronegative than hydrogen.
C) oxygen occupies more space than hydrogen.
D) hydrogen is much more electronegative than oxygen.
E) it is a hydrogen bond.
Answer: B
Objective: 9.1
Global Outcomes: GO2
2) A hydrogen bond is
A) an attraction between a hydrogen atom attached to N, O, or F and an N, O, or F atom on another molecule.
B) a covalent bond between H and O.
C) an ionic bond between H and another atom.
D) a bond that is stronger than a covalent bond.
E) the polar O-H bond in water.
Answer: A
Objective: 9.1
Global Outcomes: GO2
3) Hydrogen bonds are a major factor in the structure of
A) DNA.
B) hydrogen chloride.
C) dry ice.
D) air.
E) table salt.
Answer: A
Objective: 9.1
Global Outcomes: GO2
4) In a solution, the solvent
A) is a liquid.
B) can be a liquid or gas.
C) can be a solid, liquid, or gas.
D) is never a solid.
E) is the substance present in the smallest concentration.
Answer: C
Objective: 9.1
Global Outcomes: GO2
5) Which of the following molecules can form hydrogen bonds?
A) CH4
B) NaH
C) NH3
D) BH3
E) HI
Answer: C
Objective: 9.1
Global Outcomes: GO2
6) A solution is prepared by dissolving 2 g of KCl in 100 g of H2O. In this solution, H2O is the
A) solute.
B) solvent.
C) solution.
D) solid.
E) ionic compound.
Answer: B
Objective: 9.1
Global Outcomes: GO2
7) Oil does not dissolve in water because
A) oil is polar.
B) oil is nonpolar.
C) water is nonpolar.
D) water is saturated.
E) oil is hydrated.
Answer: B
Objective: 9.1
Global Outcomes: GO2
8) When KCl dissolves in water
A) the Cl- ions are attracted to dissolved K+ ions.
B) the Cl- ions are attracted to the partially negative oxygen atoms of the water molecule.
C) the K+ ions are attracted to Cl- ions on the KCl crystal.
D) the K+ ions are attracted to the partially negative oxygen atoms of the water molecule.
E) the K+ ions are attracted to the partially positive hydrogen atoms of the water molecule.
Answer: D
Objective: 9.1
Global Outcomes: GO2
9) Water is a polar solvent and hexane (C6H14) is a nonpolar solvent. Which of the following correctly describes the solubility of the solute?
A) mineral oil, soluble in water
B) CaCl2, soluble in hexane
C) NaHCO3, soluble in water
D) CCl4, soluble in water
E) octane, soluble in water
Answer: C
Objective: 9.1
Global Outcomes: GO2
10) In water, a substance that ionizes completely in solution is called a
A) weak electrolyte.
B) nonelectrolyte.
C) semiconductor.
D) nonconductor.
E) strong electrolyte.
Answer: E
Objective: 9.2
Global Outcomes: GO2
11) In water, a substance that partially ionizes in solution is called a
A) weak electrolyte.
B) nonelectrolyte.
C) semiconductor.
D) nonconductor.
E) strong electrolyte.
Answer: A
Objective: 9.2
Global Outcomes: GO2
12) An equivalent is
A) the amount of ion that has a 1+ charge.
B) the amount of ion that has a 1- charge.
C) the amount of ion that carries 1 mole of electrical charge.
D) 1 mole of any ion.
E) 1 mole of an ionic compound.
Answer: C
Objective: 9.2
Global Outcomes: GO2
13) How many equivalents are present in 5.0 g of Al3+?
A) 15 Eq
B) 0.56 Eq
C) 0.19 Eq
D) 0.37 Eq
E) 3 Eq
Answer: B
Objective: 9.2
Global Outcomes: GO4
14) How many equivalents are present in 5.0 moles of Al3+?
A) 15 Eq
B) 1.3 Eq
C) 5.0 Eq
D) 0.67 Eq
E) 3.0 Eq
Answer: A
Objective: 9.2
Global Outcomes: GO4
15) An intravenous replacement solution contains 4.0 mEq/L of Ca2+ ions. How many grams of Ca2+ are in 3.0 L of the solution?
A) 0.24 g
B) 0.80 g
C) 0.40 g
D) 240 g
E) 4.0 g
Answer: A
Objective: 9.2
Global Outcomes: GO4
16) How many equivalents are present in 0.40 moles of SO42-?
A) 0.10 Eq
B) 0.20 Eq
C) 0.40 Eq
D) 0.80 Eq
E) 1.2 Eq
Answer: D
Objective: 9.2
Global Outcomes: GO4
17) When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is
A) dilute.
B) polar.
C) nonpolar.
D) saturated.
E) unsaturated.
Answer: D
Objective: 9.3
Global Outcomes: GO2
18) The solubility of KI is 50 g in 100 g of H2O at 20 °C. If 110 grams of KI are added to 200 grams of H2O
A) all of the KI will dissolve.
B) the solution will freeze.
C) the solution will start boiling.
D) a saturated solution will form.
E) the solution will be unsaturated.
Answer: D
Objective: 9.3
Global Outcomes: GO4
19) An increase in the temperature of a solution usually
A) increases the boiling point.
B) increases the solubility of a gas in the solution.
C) increases the solubility of a solid solute in the solution.
D) decreases the solubility of a solid solute in the solution.
E) decreases the solubility of a liquid solute in the solution.
Answer: C
Objective: 9.3
Global Outcomes: GO2
20) Which one of the following compounds will NOT be soluble in water?
A) NaOH
B) PbS
C) K2SO4
D) LiNO3
E) MgCl2
Answer: B
Objective: 9.3
Global Outcomes: GO2
21) Which one of the following compounds will NOT be soluble in water?
A) LiOH
B) K2S
C) BaSO4
D) NaNO3
E) MgCl2
Answer: C
Objective: 9.3
Global Outcomes: GO2
22) Which one of the following compounds will be soluble in water?
A) AgCl
B) Cu(OH)2
C) LiCl
D) CaSO4
E) PbCO3
Answer: C
Objective: 9.3
Global Outcomes: GO2
23) Which one of the following compounds will be soluble in water?
A) AgBr
B) Cu(OH)2
C) NH4Cl
D) CaCO3
E) PbS
Answer: C
Objective: 9.3
Global Outcomes: GO2
24) Which one of the following compounds will be insoluble in water?
A) AgNO3
B) CaCl2
C) NH4Cl
D) CaCO3
E) Pb(C2H3O2)2
Answer: D
Objective: 9.3
Global Outcomes: GO2
25) When solutions of KCl and Pb(NO3)2 are mixed, a precipitate forms. Which of the following is the balanced equation for the double replacement reaction that occurs?
A) KCl(aq) + Pb(NO3) 2(aq) → KNO3(aq) + PbCl2(s)
B) KNO3(aq) + PbCl2(s) → KCl(aq) + Pb(NO3) 2(aq)
C) K+(aq) + NO3-(aq) → KNO3(aq)
D) 2KCl (aq) + Pb(NO3)2(aq) → 2KNO3(aq) + PbCl2 (s)
E) KCl(aq) + Pb(NO3)2(aq) → KNO3(aq) + PbCl(s)
Answer: D
Objective: 9.3
Global Outcomes: GO2
26) When solutions of NaCl and AgNO3 are mixed,
A) a precipitate of AgCl forms.
B) a precipitate of NaNO3 forms.
C) no precipitate forms.
D) precipitate of NaNO3 and AgCl form.
E) a precipitate of AgCl2 forms.
Answer: A
Objective: 9.3
Global Outcomes: GO2
27) According to Henry's law, the solubility of a gas in a liquid
A) decreases as the gas pressure above the liquid increases.
B) increases as the gas pressure above the liquid increases.
C) remains the same as the temperature increases.
D) depends on the liquid polarity.
E) depends on the liquid density.
Answer: B
Objective: 9.3
Global Outcomes: GO2
28) The mass percent concentration refers to
A) grams of solute in 1 kg of solvent.
B) grams of solute in 1 kg of solution.
C) grams of solute in 100 g of solvent.
D) grams of solute in 100 g of solution.
E) grams of solvent in 100 g of solution.
Answer: D
Objective: 9.4
Global Outcomes: GO4
29) The mass/volume percent concentration refers to
A) grams of solute in 1 L of solvent.
B) grams of solute in 1 L of solution.
C) grams of solute in 100 mL of solvent.
D) grams of solute in 100 mL of solution.
E) grams of solvent in 100 mL of solution.
Answer: D
Objective: 9.4
Global Outcomes: GO4
30) What is the concentration, in mass percent, of a solution prepared from 50.0 g NaCl and 150.0 g of water?
A) 0.250%
B) 33.3%
C) 40.0%
D) 25.0%
E) 3.00%
Answer: D
Objective: 9.4
Global Outcomes: GO4
31) Rubbing alcohol is 70.% isopropyl alcohol by volume. How many mL of isopropyl alcohol are in a 1 pint (473 mL) container?
A) 70. mL
B) 0.15 mL
C) 680 mL
D) 470 mL
E) 330 mL
Answer: E
Objective: 9.4
Global Outcomes: GO4
32) What is the concentration, in m/v percent, of a solution prepared from 50. g NaCl and 2.5 L of water?
A) 5.0%
B) 2.0%
C) 0.020%
D) 0.050%
E) 20.%
Answer: B
Objective: 9.4
Global Outcomes: GO4
33) How many grams of glucose are needed to prepare 400. mL of a 2.0%(m/v) glucose solution?
A) 800. g
B) 0.0050 g
C) 8.0 g
D) 2.0 g
E) 200. g
Answer: C
Objective: 9.4
Global Outcomes: GO4
34) A patient needs to receive 85 grams of glucose every 12 hours. What volume of a 5.0%(m/v) glucose solution needs to be administered to the patient each 12 hours?
A) 1700 mL
B) 60 mL
C) 6000 mL
D) 17 mL
E) 204 mL
Answer: A
Objective: 9.4
Global Outcomes: GO4
35) What volume (mL) of a 15% (m/v) NaOH solution contains 120 g NaOH?
A) 18 mL
B) 0.13 mL
C) 13 mL
D) 120 mL
E) 8.0 × 102 mL
Answer: E
Objective: 9.4
Global Outcomes: GO4
36) How many milliliters of a 25% (m/v) NaOH solution would contain 75 g of NaOH?
A) 25 mL
B) 75 mL
C) 33 mL
D) 19 mL
E) 3.0 × 102 mL
Answer: E
Objective: 9.4
Global Outcomes: GO4
37) What is the molarity of a solution that contains 17 g of NH3 in 0.50 L of solution?
A) 34 M
B) 2.0 M
C) 0.50 M
D) 0.029 M
E) 1.0 M
Answer: B
Objective: 9.4
Global Outcomes: GO4
38) What is the molarity of a solution that contains 3.25 moles of NaNO3 in 250. mL of solution?
A) 3.25 M
B) 6.50 M
C) 0.0130 M
D) 13.0 M
E) 2.60 M
Answer: D
Objective: 9.4
Global Outcomes: GO4
39) When 200. mL of water are added to 100. mL of 12% KCl solution the final concentration of KCl is (Assume the volumes add.)
A) 12%.
B) 4.0%.
C) 36%.
D) 6.0%.
E) 8.0%.
Answer: B
Objective: 9.4
Global Outcomes: GO4
40) The molarity (M) of a solution refers to
A) moles of solute/L of solution.
B) moles of solute/L of solvent.
C) moles of solute/100 mL of solution.
D) grams of solute/100 mL of solution.
E) grams of solute/L of solution.
Answer: A
Objective: 9.4
Global Outcomes: GO4
41) What is the molarity of a solution containing 5.0 moles of KCl in 2.0 L of solution?
A) 2.5 M
B) 1.0 M
C) 5.0 M
D) 10. M
E) 2.0 M
Answer: A
Objective: 9.4
Global Outcomes: GO4
42) What is the molarity of a solution which contains 58.5 g of sodium chloride dissolved in 0.500 L of solution?
A) 0.500 M
B) 1.00 M
C) 1.50 M
D) 2.00 M
E) 4.00 M
Answer: D
Objective: 9.4
Global Outcomes: GO4
43) How many moles of CaCl2 are in 250 mL of a 3.0 M of CaCl2 solution?
A) 750 moles
B) 1.3 moles
C) 83 moles
D) 0.75 mole
E) 3.0 moles
Answer: D
Objective: 9.4
Global Outcomes: GO4
44) What volume of a 1.5 M KOH solution is needed to provide 3.0 moles of KOH?
A) 3.0 L
B) 0.50 L
C) 2.0 L
D) 4.5 L
E) 0.22 L
Answer: C
Objective: 9.4
Global Outcomes: GO4
45) How many grams of PbCl2 are formed when 25.0 mL of 0.654 M KCl react with Pb(NO3)2?
2KCl(aq) + Pb(NO3) 2(aq) → 2KNO3(aq) + PbCl2(s)
A) 22.7 g
B) 1.64 g
C) 2.27 g
D) 4.54 g
E) 9.08 g
Answer: C
Objective: 9.4
Global Outcomes: GO4
46) How many mL of 0.246 M Pb(NO3)2 are needed to react with 36.0 mL of 0.322 M KCl ?
2KCl(aq) + Pb(NO3) 2(aq) → 2KNO3(aq) + PbCl2(s)
A) 36.0 mL
B) 18.0 mL
C) 72.0 mL
D) 47.1 mL
E) 23.6 mL
Answer: E
Objective: 9.4
Global Outcomes: GO4
47) Use the reaction: 2AgNO3(aq) + H2SO4(aq) → Ag2SO4(s) + 2H2O(l).
What volume of 0.123 M AgNO3(aq) is needed to form 0.657 g of Ag2SO4(s)?
A) 34.2 L
B) 17.1 mL
C) 34.3 mL
D) 10.7 mL
E) 53.4 mL
Answer: C
Objective: 9.4
Global Outcomes: GO4
48) During the process of diluting a solution to a lower concentration,
A) the amount of solute does not change.
B) the amount of solvent does not change.
C) there is more solute in the concentrated solution.
D) the volume of the solution does not change.
E) water is removed from the concentrated solution.
Answer: A
Objective: 9.5
Global Outcomes: GO2