Introduction to Acids and Base Equilibria
Name: ______________________Period:____
AP Chemistry
Address qll MC questions and submit to Response System
1.
5.
CH3NH2 + H2O « CH3NH3+ + OH–
Which species acts as an acid?
I. H2O II. CH3NH 3+ III. CH 3NH 2
A) I only
C) I and II only
E) I, II, and III
Based on the above table, list the acids in order of increasing acid strength.
A)
B)
C)
D)
E)
6. The conjugate base of H 2BO 3– is
A) BO 33–
C) H2BO 3–
E) HBO32–
CH 3COOH, NH 4+ , HIO 3
HIO 3, CH 3COOH, NH 4+
HIO 3, HIO 3, CH 3COOH
NH 4+ , HIO 3, CH 3COOH
NH 4+ , CH 3COOH, HIO 3
B) H2BO 4–
D) H3BO 3
7. All of the following ions can act as Bronsted-Lowry
acids in solution EXCEPT
2. Base your answer to the following question on A few
drops of the indicator bromothymol blue [HBb] is added
to water
HBb(aq) + H2O( ) H3O+ (aq) + Bb –(aq)
Yellow Blue
A) HPO 42–
C) SO 42–
E) CH 3COOH
B) H2O
D) NH 4+
8. Which is amphiprotic?
A) SO 32–
C) PO 43–
E) HCl
Which statement is correct? The addition of
A) KOH(aq) causes the [HBb] to increase and the
solution to turn yellow.
B) HCl(aq) causes the [H 3O+ ] to decrease and the
solution to turn yellow.
C) HCl(aq) causes an equilibrium shift toward the
reactants and the solution turns blue.
D) KOH(aq) causes an equilibrium shift toward the
products and the solution turns yellow.
E) HCl(aq) causes the [H3O + ] to increase and the
solution to turn yellow.
3. Which of the following 0.10 M solutions is basic?
A) LiCl
C) NaClO 4
E) HCl
B) II only
D) II and III only
B) K 3PO 4
D) NH 4NO 3
4. Which of the following is possible for an acid?
A) Acid strength: strong; Concentration: 0.01 M;
pH: 2.0
B) Acid strength: weak; Concentration: 0.01 M; pH: 1.0
C) Acid strength: strong; Concentration: 3 M; pH: 5.5
D) Acid strength: weak; Concentration: 3 M; pH: –0.5
E) Acid strength: strong; Concentration: 1 M; pH: 6.5
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B) NH 4+
D) HSO3–
Base your answers to questions 9 through 12 on the
titration diagram below.
14. A beaker containing 50. mL of 0.1 M H2SO 4 is added
to a flask containing 150. mL of 0.2 M NaOH. What is
the [ H+] in the flask after mixing?
A) 8 × 10 –14 M
C) 1 × 10 –7 M
E) 1 × 10 –26 M
B) 1 × 10 –13 M
D) 1 × 10 –1 M
15. Which of the following is something not to do, or is
unnecessary when performing a titration?
A) Keeping the solution well mixed by constant
stirring
B) Rinsing the beaker that is to hold the solution
to be titrated right before pouring the solution
in
C) Draining the pipet by touching the tip to the side
of the container that is catching
D) Turning the stopcock immediately so that the
titration stops when the indicator changes color
E) Keeping track of the volume of the solution in the
buret both at the beginning of the experiment and
after the titration
9. This point is the equivalence point.
A) I
C) III
E) I and III
B) II
D) IV
10. This is when there is excess base.
A) I
C) III
E) II and IV
B) II
D) IV
11. The pH of the solution is equal to the pKa of the acid.
A) I
C) III
E) II and IV
B) II
D) IV
16.
12. At this point the solution is buffered.
A) I
C) III
E) II and IV
HClO(aq) = H+(aq) + ClO –(aq)
The pH of a 0.025 M solution of hypochlorous acid,
HClO, is 3.0. What is the K a for HClO at this
temperature?
A) 2.5 × 10 –8
C) 4.0 × 10 –7
E) 2.0 × 10 –3
B) II
D) IV
B) 2.5 × 10 –7
D) 4.0 × 10 –5
17. What is the H + (aq) concentration in a 0.01 M
concentration of HClO(aq) (K a = 3.00 × 10 –8)?
13.
A) 1.73 × 10 –4
C) 1.73 × 10 –5
E) 17.3 × 10 –5
B) 9.00 × 10 –20
D) 3.00 × 10 –10
18. What is the pH of a solution prepared by adding 60.0
mL of 0.150 M HCl to 140.0 mL of 0.100 M KOH?
A) 1.60
Which indicator is used for the titration represented by
the above titration curve?
A) Alizarin yellow
C) Phenolphthalein
E) None of these
B) Methyl red
D) Thymolphthalein
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B) 2.80
C) 3.20
D) 8.20
E) 12.40
19.
Solution A: [OH–] = 5.0 × 10–11 M
Solution B: [H+] = 0.20 M
Solution C: pOH = 11.30 Solution D: pH = 1.20
23. If temperature is increased, the [SO 3]
A) A
Four monoprotic acids of the same concentration are
labeled above.
List the four solutions above in order of DECREASING
acidity.
A) D > B > C > A
C) A > B > C > D
E) D > C > B > A
21.
A) k = [A][B]
C) k = [A][B]2
E) k = [A][B]2
2 SO 2(g) + O2(g) « 2 SO 3(g) + 46.8 kcal
(A) increases
(B) decreases
(C) remains the same
(D) increases, then decreases
(E) decreases, then increases
22. If temperature is decreased, the Keq
D) D
Cl2(l) + 2 Na(s) ® 2 NaCl(s)
The reaction rate can be significantly increased by:
A)
B)
C)
D)
E)
B) a base
D) an inert medium
C) C
B) k = [A] 2[B]
D) k = [A] 2[B] 2
25. Given the reaction:
Base your answers to questions 22 and 23 on the
equation and the choices provided.
B) B
E) E
What is the rate law for this equation?
HSO4– + H2O ® H3O+ + SO42–
In the above reaction between the hydrogen sulfate ion
and water, the water acts as
A) A
D) D
B) C > D > B > A
D) B > D > C > A
B) KNH2
D) NH 4Cl
A) an acid
C) a salt
E) a catalyst
C) C
24. An experiment was conducted to determine the rate law
of the reaction 2 A + 2 B ® C + D. The data collected
is shown below.
20. Which will produce a buffer solution when added to 1.0
M NH 3?
A) HNO3
C) NaOH
E) K3PO 4
B) B
E) E
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cooling the system
adding more sodium, Na
increasing the volume of the system
removing sodium chloride, NaCl
using gaseous chlorine, Cl2
Answer Key
Acids and Bases
1.
E
2.
E
3.
B
4.
A
5.
C
6.
E
7.
C
8.
D
9.
C
10.
D
11.
B
12.
B
13.
B
14.
B
15.
B
16.
D
17.
C
18.
E
19.
D
20.
D
21.
B
22.
A
23.
B
24.
D
25.
E
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