Download Acids and Bases - Parkway C-2

Acids and Bases Review
Honors Chemistry
For the following reactions, classify them as:
o acid ionization
o base ionization
o proton transfer
o neutralization
(you may have more than one answer for a reaction)
1)
2)
NaOH  Na+
3KOH
+
+ OH-
H3PO4  K3PO4 + 3H2O
3)
HSO4- + S2-  HS- + SO42-
4)
NH3 + H2CO3  NH4+ + HCO3-
5)
Ba(OH)2 + H2S  BaS + H2O
6) Explain why the Bronsted-Lowry acid/base definition is broader than the Arrhenius one.
Use an example of a reaction to illustrate this.
7) What is the pH of a 3.90 x 10-3 M solution of calcium hydroxide?
8) How many grams of sulfuric acid are there in a 200. mL solution which has a pH of 1.05?
9) What concentration of hydroxide exists within a .0089 M concentration of hydrobromic
acid?
10) Use Ka to find the pH of a .0135 M solution of acetic acid.
11) What is the molarity of a solution of KOH if 22.9 mL of it are needed to neutralize 44.0
mL of 2.05 x 10-4 M phosphoric acid.
12) What volume of .080 M calcium hydroxide is needed to neutralize 60.0 mL of 2.80 x 10-2
M hydrosulfuric acid?
13) Ascorbic acid (vitamin C) is a diprotic acid. What is the pH of a 0.95 M solution of
ascorbic acid? Also determine the equilibrium concentration of the ascorbate ion (Asc2-).
Ka1 = 7.9 x 10-5 and Ka2 = 1.6 x 10-12
pH = ________ [Asc2-] = ____________
14) What would you expect the pH to be for a combination of 84.5 mL of .65 M HI (strong
acid) and 68.0 mL of .48 M Sr(OH)2 (strong base)?
pH =
____________
15) Calculate the pH at the equivalence point for a titration of 30.0 mL of .75 M LiOH
(strong base) with .80 M pyruvic acid (Ka = 1.4 x 10-4).
pH =
____________
16) What would be the pH of a 1.0 L solution of 0.25 M HCHO2 (formic acid – Ka = 1.7 x 10-4)
to which 70.00 g of KCHO2 is added (assume all of the potassium formate dissolves).
pH = ____________
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. What are the acids in the following equilibrium reaction?
CN + H O
HCN + OH
a. CN , H O
c. CN , OH
b. H O, HCN
d. H O, OH
____
2. Which of the following represents a Brønsted-Lowry conjugate acid-base pair?
a. SO
c. H O and H
and SO
b. CO
d. NH and NH
and CO
____
3. Which of these solutions is the most basic?
a. [H3O ] = 1 10 M
c. [H3O ] = 1 10 M
b. [OH ] = 1 10 M
d. [OH ] = 1 10 M
4. An indicator is what type of compound?
a. oxidizing agent
c. strong base or acid
b. weak base or acid
d. salt
5. What characterizes a strong acid or base?
a. polar covalent bonding
b. complete ionization in water
c. ionic bonding
d. presence of a hydroxide or hydrogen ion
6. With solutions of strong acids and strong bases, the word strong refers to ____.
a. normality
c. solubility
b. molarity
d. degree of ionization
7. Fewer than 1% of acetic acid molecules are ionized at any instant. The acetate ion is therefore
____.
a. a poor proton acceptor
c. a poor hydrogen-ion donor
b. a good hydrogen-ion acceptor
d. a good hydrogen-ion donor
____
____
____
____
____
8. A substance with a K of 1 10
a. strong acid
b. weak acid
____
9. The ionization constant (K ) of HF is 6.7
solution of this acid?
a. [HF] is greater than [H3O ][F ].
b. [HF] is less than [H3O ][F ].
____ 10. The K of carbonic acid is 4.3
would be classified as a ____.
c. strong base
d. weak base
10 . Which of the following is true in a 0.1M
c. [HF] is equal to [H3O ][F ].
d. [HF] is equal to [H3O ][F ].
10 .
H CO + H2O
H3O + HCO
This means that H CO is a ____.
a. good proton acceptor
b. poor proton acceptor
c. good proton donor
d. poor proton donor
acid base review questions - honors
Answer Section
MULTIPLE CHOICE
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
B
D
C
B
B
D
B
B
A
D