Chapters 14-15: Acid – Base Review
Name ___KEY___________ Per___
Use another sheet of paper to complete the following:
1. Rank 1M solutions of the following in order of increasing hydrogen ion concentrations:
weak acid
strong acid
strong base weak base
3
4
1
2
2. Define the following:
a) Arrhenius acid
d) Arrhenius Base
b) Bronsted – Lowry Acid
e) Bronsted – Lowry Base
c) Lewis Acid
f) Lewis Base
3. Why does a proton transfer reaction favor the weaker side?
The weaker side cannot compete successfully with the stronger side. For example, a
strong acid dissociates readily due to the weak attraction between the H+ and the anion.
The conjugate base (the anion) will not have a strong attraction for the H+, so the reverse
reaction (to the stronger side) is much less likely to take place.
4. Use Table 14.6 in your textbook to rank the following acids from weakest to strongest:
NH4+
HCO3H2PO4H2O
3
2
4
1
5. Write the equilibrium equation for the following weak acids:
a) H2S
b) NH4+
c) C6H5COOH
+
a) H2S + H2O ↔ HS + H3O
b) NH4+ + H2O ↔ NH3 + H3O+
c) C6H5COOH + H2O ↔ C6H5COO- + H3O+
6. Match each solution with its correct description.
_4_ a. dilute, weak acid
_2_ b. dilute, strong base
_1_ c. concentrated, strong acid
_5_ d. dilute, strong acid
_3_ e. concentrated, weak base
(1) 18M H2SO4(aq)
(2) 0.5 M NaOH(aq)
(3) 15 M NH3(aq)
(4) 0.1 M HC2H3O2(aq)
(5) 0.1 M HCl(aq)
7. Classify the following as monoproctic, diproctic, or triprotic.
a) HCOOH
b) HBr
c) H2SO3
monoproctic
monoproctic
diproctic
d) H3C6H5O7 (citric acid)
triproctic
8. What would you expect to happen when lithium metal is added to water? Write the balanced
chemical equation.
2Li(s) + 2H2O(l)  2LiOH(aq) + H2(g)
Chapters 14-15: Acid – Base Review
Name ___KEY___________ Per___
9. Classify each solution as acidic, basic, or neutral:
__basic_ a. [H+] = 2.5 X 10-9 M
__acidic_ b. pOH = 12.0
__acidic_ c. [OH-] = 9.8 X 10-11 M
_neutral_ d. [H+] = 1 X 10-7 M
__acidic_ e. pH = 0.8
__basic__ f. [OH-] = 1.7 X 10-2 M
10. A solution has a pOH of 12.4. What is the pH of this solution?
pH = 1.6
11. Identify the hydrogen ion donor(s) and hydrogen ion acceptors for the ionization of sulfuric
acid in water. Label the conjugate acid-base pairs.
H2SO4 + H2O (l)  HSO4- + H3O+
Donor acceptor acceptor donor
Pairs: 1) H2SO4 and HSO4- 2) H2O and H3O+
12. Write the step-by-step dissociation equations for phosphoric acid. Identify all the ions that
form when the acid dissociates.
(1) H3PO4 + H2O(l) ↔ H2PO4-(aq) + H3O+(aq)
(2) H2PO4-(aq) + H2O(l) ↔ HPO42-(aq) + H3O+(aq)
(3) HPO42-(aq) + H2O(aq) ↔ PO43-(aq) + H3O+ (aq)
Dihydrogen phosphate
Monohydrogen phosphate
Phosphate
Hydronium ion (x3)
-5
13. Calculate the pH if the hydrogen ion concentration is 4.73 X 10 M.
pH = 4.3
14. Calculate the hydroxide ion of the pH of 8.25.
1.8 x 10-6 M
15. Write an equation for the ionization of acetic acid in water. Label the acid, base,
conjugate acid, and conjugate base.
CH3COOH + H2O(l) ↔ CH3COO-(aq) + H3O+(aq)
Acid
base
conj. Base
conj.acid
16. Define amphoteric and give two examples of substances that are amphoteric.
A substance that can behave as an acid or a base e.g. HCO3-, HPO42-, HSO417. A 0.130 M solution of acetic acid has a hydronium ion concentration of 1.53 X 10-3M.
Calculate the pH of the acid.
pH = 2.815
18. Complete and balance the chemical equations fo the following reactions:
a) 2K(s) + 2H2O(l)  2KOH(aq) + H2(g)
Chapters 14-15: Acid – Base Review
Name ___KEY___________ Per___
b) 2HClO3 + Be(OH)2(aq)  Be(ClO3)2(aq) + 2H2O
c) BaO(s) + H2O(l)  Ba(OH)2
d) 2H3PO4 + 3Mg(OH)2  Mg3(PO4)2(aq) + 6H2O(l)
e) HNO3 + NH3(g)  NO3-(aq) + NH+(aq) OR HNO3(aq) + NH4OH(aq)  NH4NO3(aq) + H2O(l)
f) H2CO3(aq) + NH3(g)  NH4+(aq) + HCO3-(aq)
OR
H2CO3(aq) + 2 NH4OH(aq)  (NH4)2CO3(aq) + 2H2O(l)
g) BaCO3(s) + 2HCl(aq)  BaCl2(aq) + CO2(g) + H2O(l)
21. A 50.0 mL sample of nitric acid is titrated to its end point with 25.2 mL of 2.50 M KOH.
What is the concentration of the acid?
1.26 M
22. What is the molarity of a NaOH solution if 38.0 mL of the solution is titrated to its end
point with 14.0 mL of 0.750 M sulfuric acid?
0.553 M
23. What volume of 0.12 barium hydroxide is needed to neutralize 12.2 mL of 0.25 M HCl?
13 mL
24. An ammonia-based cleaner with a volume of 65.5 mL was neutralized with 16.2 mL of 1.20
M HNO3. What is the molarity of the ammonia in the cleaner?
0.297 M
25. A cleaner containing NaOH with a volume of 35.2 mL was neutralized with 25.4 mL of 2.50
mL sulfuric acid. Calculate the molarity of the NaOH in the cleaner.
3.61 M
26. What is the molarity of 55.3 mL of sulfuric acid if it is titrated to its end point with 122.7 mL
of 0.75 M calcium hydroxide?
1.7 M
27. What is the formula for the conjugate base from the following?
a) HCN
b) N2H5+
c) H3AsO4-
CNN2H4
H2AsO42-
28. What is the formula of the acid or base formed when each of the following is added to water?
a) Cs2O
CsOH
b) SO2
H3SO3
Chapters 14-15: Acid – Base Review
Name ___KEY___________ Per___
29. Write the formula of the salt formed when a solution of LiOH is added to a solution of H3PO4.
Li3PO4
30. 31.4 mL of 2.76 M HCl neutralizes 37.8 mL of Ba(OH)2. Find the concentration of the base.
1.15 M
31. What volume of 0.107 M NaOH will neutralize 22.3 mL of 0.424 M HClO4?
88.4 mL
32. What is the pH of a 0.370 M HI solution?
pH = 0.432
-3
33. Determine the pH of a 1.1 X 10 M Ba(OH)2 solution.
pH = 11.34
34. Find the hydronium ion concentration in a water solution when the hydroxide concentration
is 2.98 X 10-5 M.
3.36 X 10-10 M