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1. Consider the reaction: 2HgO(s) ⇄ 2Hg(l) + O2(g)
which of following will shift the equilibrium toward the reactants? I) more solid HgO is added;
II) decreasing the pressure;
III) more O2 is added
  1. I and III
  2. II only
  3. I, II and III
  4. III only
NO2(g) + CO(g) ⇄
2. Consider the reaction:
A 1L vessel at 400C contains the equilibrium concentrations [NO] = 0.1 M, [CO2]= 0.02 M, [NO2] = 0.01 M, and [CO] = 0.1M. What is the value of the equilibrium constant Kc for the reaction?
a. 0.5 
b. 5 
c. 1 
d. 2


3. Determine the pH of a 5.5 ×10−2M solution of H2SO4. 
a. 1.25
b. 0.95
c. 7.00
d. 6.48


4. Which of the following mixtures can produce a buffer?
  1. CH3COOH, CH3COONa
  2. H++OH−
  3. HCl + NaOH
  4. all of the above
5. The pH of a solution changes from 5.1 to 8.1.This indicates that the [OH−] of the solution has:
  1. increased by 3 M
  2. decreased by 3 M
  3. increased by a factor of 1000
  4. decreased by a factor of 100
6. If the pH of HNO3 solution is 2.45, what is the molarity of this solution?
  1. 3.5 × 10−3M
  2. 2.45 × 10−5 M
  3. 2.81×102M
  4. Can’t be calculated
7. Consider the dissociation of hydrofluoric in water. What is the conjugate base to the acid?
a. F-
  1. H2O+
  2. H3O
  3. Can’t be determined
8. A solution with a hydronium concentration of a 10-6 M is:
  1. basic
  2. acidic
  3. neutral
  4. None of the above
9. Which of the following is a strong acid?
  1. Nitrous acid
  2. Acetic acid
  3. Sulfuric acid
  4. water
10. What is the pH of a 1x10-4M KOH solution? 
a. 4.00
b. 10.00
c. 6.00
d. 7.00
14. A solution with [H+] = 5 x10-11 M would have a pH ------and would be considered -------
  1. between 1 and 2; acidic
  2. between 10 and 11; basic
  3. 2; basic
  4. 2; acidic
15. The titration of 25.0 mL of 0.125 M H2SO4 solution required 27.07 mL of KOH to reach
the endpoint. What is the concentration of the KOH? a) 0.115 M
b) 0.230 M
c) 0.169 M
d) 0.0848 M 
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