Wesley Minor
Mock Exam 4
1. Which of the following may describe a base?
i. When dissolved in water, the solution has a pH less than 7.
ii. When dissolved in water, may donate a hydroxide ion
iii. When dissolved in water, may donate a hydrogen ion
iv. When dissolved in water, may accept a hydrogen ion
v. When dissolved in water, has a pH greater than 7
A. i and iv
B. ii and v
C. ii and iii
D. ii, iv, and v
E. ii, iii, and v
2. How does a catalyst speed up the rate of reaction?
A. By increasing the rate at which reactants and products come together
B. By increasing the heat of reaction
C. By decreasing the activation energy of a reaction
D. By removing reactants from the chemical reaction
E. By increasing the energy of the products
3. Which of the following statements are true regarding strong electrolytes?
i. Strong electrolytes are insoluble in water
ii. Strong electrolytes form a solution in water
iii. Strong electrolytes are poor conductors of electricity
iv. Strong electrolytes are made up of ions
v. Hydrochloric acid is a strong electrolyte
A. i and ii
B. iii and iv
C. ii, iii, and v D. i and iii
E. ii, iv, and v
4. Assuming an exothermic reaction is reversible, how would heating likely affect the
reaction?
A. The equilibrium would shift toward products B. The heat of reaction would increase
C. The equilibrium would not change D. The activation energy would decrease
E. The equilibrium would shift toward reactants
5. What is the pH of a solution with [H3O+] = 0.00535?
A. 1.35 B. 2.27 C. 5.35 D. 12.65 E. 11.73
6. What is the pH of a solution with [OH-] = 0.00789?
A. 2.10 B. 11.90 C. 4.56 D. 9.44 E. 12.89
7. A 4.00 gram sample of NaOH is dissolved in enough water to make 0.50 liter of solution.
What is the pH?
A. 13.30 B. 0.69 C. 0.90 D. 13.10 E. 1.78
Wesley Minor
Mock Exam 4
8. Which of the following is true about a reaction when a catalyst is added to the system?
a. Equilibrium will shift to the products.
b. Equilibrium will shift to the reactants.
c. Equilibrium will shift to lower the heat.
d. No effect on the equilibrium.
Consider the following reaction for questions 9-11
N2 + H2  NH3 + 22.1 kcal
9. What is the Kc if the N2 and H2 concentrations are 0.4 and NH3 is 0.8?
A. 25 B. 7.8 C. 0.64 D. 1.6 E. 2
10. What is the Kc if H2 were a liquid?
A. 25 B. 7.8 C. 0.64 D. 1.6 E. 2
11. What is the Kc if H2 and N2 were a liquid?
A. 25 B. 7.8 C. 0.64 D. 1.6 E. 2
12. What is Kw?
A. 6.626 x 10 -34 B. 2.99 x 108 C. 6.022 x 10 -23 D. 1 x 10 -14
13. What is the conjugate base for CH3COOH?
A. CH3COO- B. CH3CO- C. CH4COO- D. CH3COOH2
14. Which of the following is a strong acid?
A. NaOH B. H2SO4 C. LiOH D. HF
15. What is used in titrations to determine the endpoint?
A. Electrode B. indicator C. litmus paper D. reaction rate
16. What is the pH of a solution with [Acid] = 2.8 [base] = 9.3 & ka= 1.89 x 10-5 ?
A. 5.244 B. 5.897 C. 4.202 D. 4.473
17. Titration reveals that 11.6 mL of 3.0 M sulfuric acid are required to neutralize the
sodium hydroxide in 25.00 mL of NaOH solution. What is the molarity of the NaOH
solution?
H2SO4(aq) + NaOH(aq) → H2O(l) + Na2SO4(aq)
A. 2.5 M
B. 3.1 M
C. 2.8 M
D. 4.7 M