Chem12 Acid Base (Unit 5) Practice Test
D1) Identify acids and bases through experimentation
1. Which of the following are properties of acids only, bases only, or both?
a. conduct electricity when in water
b. react with some metals to produce hydrogen gas
c. feel slippery
d. turn litmus red
e. taste sour
2. Which of the following represents the results of tests using an acidic solution?
A
B
C
D
Reaction with Mg(s)
Litmus
yes
red
yes
no
no
blue
blue
red
3. Which of the following conduct electricity? (Choose all that apply)
A. HCl
B. NH3
C. CH4
D. KOH
D2) Identify various models for representing acids and bases
4. Which equation represents the behaviour of a strong Arrhenius base?
A. CaO(s) + H2O( l) ← → Ca(OH)2(s)
B. RbOH(aq) → Rb+ (aq) + OH− (aq)
C. Co(OH)2 (s) →Co2+(aq) + O2(g) + H2(g)
D.Al(H2O)63+(aq ) + H2O(l) ←→Al(H2O)5(OH)2+(aq) + H3O+(aq)
5. Explain the Arrhenius and Bronsted Lowry theories, noting similarities and differences.
6. What is a characteristic common to all strong acids?
A. They ionize 100%.
B. They are concentrated.
C. They only react with strong bases.
D. They have strong conjugate bases.
6. Identify the reactant acid and its conjugate base in the equilibrium below.
Al (H2O)63+ + HS - ← → H2S + Al(H2O)5(OH)2+
7. Given the equilibrium:
HCO3− + NH4+ ← → H2CO3 + NH3
Which species is the Brønsted-Lowry base for the forward reaction?
A. NH3
B. NH4+
C. HCO3−
D. H2CO3
8. What is the conjugate acid and conjugate base of HPO42-?
D3) Analyse equations representing the reaction of acids or bases with water
9. What is formed when NH2− reacts with water?
A. H3O+
B. NH4+
C. NH3
D. NH2 −
10. Write the predominant reactions of the following in water:
a. H2SO4
b. HSO3c. CN-
d. K2O
D4) Classify an acid or base in solution as either weak or strong
11. What is the difference between a strong base and a weak base? How could you determine the
difference between a 0.1 M strong base and a 0.1 M weak base in a lab setting?
12. Which of the following is the weakest acid?
A. 0.10M CH3COOH
B. 0.50M HClO4
C. 1.0M HIO3
D. 1.5M HCN
13. Which of the following is the correct sequence of relative acid strengths?
A. HO2-> HCO3-> H2O2> H2CO3
B. H2CO3> HCO3 -> H2O2> HO2C. H2CO3> H2O2> HCO3-> HO2D. HCO3-> H2O2> H2CO3> HO2-
14. Rank the following acids in order from most to least H3O+ present in an aqueous solution:
1.0M HI
1.0M HF
1.0M HCl
1.0M H2S
1.0M H3PO4
D5) Analyse the equilibria that exist in weak acid or weak base systems
15. What is the reaction for the predominant equilibrium in HPO 42− (aq)?
16. Water reacts most completely as an acid with which of the following?
A. HO2B. CO32C. C2O42D. HPO42D6) Identify chemical species that are amphiprotic
17. What does amphiprotic mean? How do you know if a species is amphiprotic?
18. Which of the following are amphiprotic?
H2O
PO43-
H2SO3 NH2-
HC2O4-
E1) Analyse the equilibrium that exists in water
19. Which of the following equations represents the ionization of water?
A.H2O( l) ←→ H2 (aq) + O2 (aq)
B.H2O( l) ←→ H+ (aq) + OH− (aq)
C.2H2O( l) ←→ H3O+ (aq) + O2− (aq)
D.2H2O( l) ←→ H3O+ (aq) + OH− (aq)
20. The ionization of water is endothermic. Which of the following is a reasonable value of Kw
if the temperature of water is greater than 25ºC ?
A. 1.2 × 10−15
B. 0.81 × 10−14
C. 1.0 × 10−14
D. 2.0 × 10−14
E2. Perform calculations relating pH, pOH, [H3O+], and [OH-]
21. Which of the following 0.10M solutions would have the highest pH?
A. H2S
B. HIO3
C. HNO2
D. CH3COOH
22. What is the pOH of 0.25M HNO3?
A. 4.0 × 10−14
B. − 0.60
C. 0.60
D. 13.40
23. Calculate the pH, [OH-], and [H3O+] for a basic solution with a pOH of 9.54.
E3) Explain the significance of the Ka and Kb equilibrium expressions
24. What is the equilibrium constant expression for the predominant equilibrium in HCO 3- (aq) ?
25. You have two acids, a 1M solution with a Ka of 1x10-5 and a 1M solution with a Ka of 5x10-7. Which
solution contains the greater concentration of H 3O+?
E4) Perform calculations involving Ka and Kb
26. Calculate the pOH of a 1.5M solution of HF
27. Aniline (C6H5NH2- ) is a weak base with a Kb = 4.3x 10-10
Calculate the concentration of an aniline solution that has a pH = 8.80 .
Begin by writing the equation for the predominant equilibrium.