Chapters- 10
Multiple-Choice Questions
1) A solution is prepared by dissolving 2 g of KCl in 100 g of H 2 O . In this solution, H 2 O is the
A) solute.
B) solvent.
C) solution.
D) solid.
E) ionic compound.
2) 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.
3) 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.
4) Water is a polar solvent and hexane ( C 6 H 14 ) is a nonpolar solvent. Which of the following
correctly describes the solubility of the solute?
A) mineral oil, soluble in water
B) Ca Cl 2 , soluble in hexane
C) NaHCO 3 , soluble in water
D) CCl 4 , soluble in water
E) octane, soluble in water
5) In water, a substance that ionizes completely in solution is called a
A) weak electrolyte.
B) nonelectrolyte.
C) semiconductor.
D) nonconductor.
E) strong electrolyte.
6) 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.
7) 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.
8) The solubility of KI is 50 g in 100 g of H 2 O at 20 °C. If 110 grams of KI are added to 200
grams of H 2 O,
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.
9) 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.
10) The mass/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.
11) In the process known as osmosis, ________ moves through a semipermeable membrane into
an area of ________ concentration.
A) solute, lower solute
B) solute, higher solute
C) solvent, lower solute
D) solvent, lower solvent
E) solvent, higher solvent
12) What is the molarity of a solution that contains 17 g of NH 3 in 0.50 L of solution?
13) 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.
1) Which of the following is not a common characteristic of an acid?
a) it turns litmus pink/red
b) it tastes bitter
c) it dissolves common metals
d) all of these choices are common characteristics of acids
14) Which of the following is not a common characteristic of a base?
a) it turns litmus pink/red
b) it feels slippery
c) it tastes bitter
d) all of these choices are common characteristics of bases
15) A conjugate acid-base pair
a) is related by the loss and gain of H+ between 2 corresponding compounds on opposite sides of
the reaction arrow.
b) has the base donating an H+ to form its conjugate base.
c) has the acid donating an H+ to form its conjugate acid.
d) is not related in any way.
16) Which of the following is the conjugate acid of NH3?
a) NH2b) NH4+
c) HNO3
d) H3O+
17) In the reaction:
HNO2 + H2O
H3O+ + NO2-
The conjugate acid of water is ___.
a) HNO2
b) H2O
c) H3O+
d) NO2a) The concentration of reactants is greater than the concentration of the products.
b) The concentration of products is the same as the concentration of reactants.
c) The concentration of the products is greater than the concentration of the reactants.
d) Relative composition of reaction mixture cannot be predicted.
18) The equation:
C(s) + O2(g)
CO2(g)
has the following equilibrium constant expression.
[C][O 2 ]
[CO 2 ]
[CO 2 ]
b) K eq 
[O 2 ]
[O 2 ]
c) K eq 
[CO 2 ]
[CO 2 ]
d) K eq 
[C][O 2 ]
a) K eq 
19) The equilibrium constant, Keq, for the ammonia synthesis below is found to be 6.0 x 10-2 at
500C. Which of the following statements is true at equilibrium?
N2(g) + 3H2(g)
2NH3(g)
a) Product concentration is greater than reactant concentration.
b) Reactant concentration is greater than product concentration.
c) Reactant concentration is the same as product concentration.
d) Relative concentrations of reactants and products cannot be predicted.
20) The equilibrium constant Keq for the reaction of molecular hydrogen and molecular iodine in
the gas phase is 54.3 at 430C.
H2 (g) + I2(g)
2HI(g)
Which of the following statements is true for this reaction at equilibrium?
a) The reactant concentration is larger than the product concentration.
b) The product concentration is larger than the reactant concentration.
c) The reactant concentration is the same as the product concentration.
d) None of these answer choices are correct.
21) When stress is applied to a system at equilibrium such that the equilibrium is disturbed, the
reaction proceeds in the direction that counteracts the disturbance. This explanation best
describes ___.
a) Brønsted-Lowry concept
b) Ion-Ion attraction
c) Conjugate pair analysis
d) Le Châtelier’s principle
22) Which of the conditions below would drive this reaction to the right?
H
H
H
C
O
C
O
C
O
H +
H3O+
H
pyruvic acid
H
H
O
O
C
C
C
H
H
O
H + H2O
lactic acid
a) removing hydronium ion
b) adding lactic acid
c) adding water
d) adding pyruvic acid
23) What is the concentration of [H3O+] in an aqueous solution when the [OH-] is 5.2 x 10-9 M?
a) 1.9 x 10-6 M
b) 5.7 M
c) 1.0 x 10-14 M
d) 9.8 x 10-9 M
24) Kw, the equilibrium constant for the ionization of water by the equation below, is 1.0 x 10-14.
What does that mean when we are considering pure water?
+
H3O + OH
2H2O
a) More ions exist than water molecules.
b) The majority of the molecules present are in the form of H2O.
c) The amount of water is the same as the amount of the ions present.
d) There will always be more hydronium ions present than water at equilibrium.
25) A solution in which the concentration of H+ is greater than the concentration of OH- will
a) have a pH greater than 7.0 and be basic.
b) have a pH less than 7.0 and be basic.
c) have a pH greater than 7.0 and be acidic.
d) have a pH less than 7.0 and be acidic.
26) When one is referring to pH, what is the meaning of the p?
a) Take the log of the number.
b) Multiply the p constant by the number.
c) Take the negative log of the number.
d) All are possible depending on the number following the p.
27) Calculate the pH of solution produced by dissolving 0.001 moles of HNO3 in a liter of water.
Assume complete dissociation.
a) pH = 3.0
b) pH = 0.001
c) pH = 1 x 10–3
d) pH = 1 x 103
28) What is the molar concentration of hydronium ions in a sample of a soft drink that has a pH
of 4?
a) 1/4 M
b) 4 M
c) 1 x 104 M
d) 1 x 10-4 M
29) A Ka can be calculated for some chemical reactions. The Ka is
a) the Keq for the reaction to the right.
b) the Keq for the reaction to the left.
c) the Keq for the dissociation of an acid.
d) the pH of a very weak solution.
30) Which of the following statements is true?
a) The larger the Ka for an acid, the weaker the acid.
b) The smaller the pKa of an acid, the stronger the acid.
c) The larger the pKa of an acid, the stronger the acid.
d) The smaller the Ka, the stronger the acid.
31) 15.00 mL of 0.100 M NaOH is required to completely neutralize 25.00 mL of an HCl
solution. What is the concentration of the HCl solution?
a) 0.0600 M
b) 0.100 M
c) 0.167 M
d) 1.50 M
32) The pH of blood is held reasonably stable by which buffer system?
a) H3PO4/H2PO4–
b) NaCl/Cl–
c) H2CO3/HCO3–
d) HCl/Cl–
33) Antacids may contain which ion to reduce acidity?
a) Na+
b) CO32–
c) Al3+
d) Cl–
34) 15.00 mL of 0.100 M NaOH is required to completely neutralize 25.00 mL of an HCl
solution. What is the concentration of the HCl solution?
a) 0.0600 M
b) 0.100 M
c) 0.167 M
d) 1.50 M
35) Calculate the pKa of water whose Ka is 1.8 x 10-16.