1. Calculate the pH of a solution that is 0.2 M in acetic acid (K = 1.8 x 10-5) and 0.2 M in sodium acetate.

A) 7.0  B) 4.7   C) 9.3  D) 8.6   E) 5.4

2. The equilibrium constants (Ka) for HCN and HF in H2O at 25°C are 6.2 x 10-10 and

7.2 x 10-4, respectively.The relative order of base strengths is:

A) CN->F->H20

B) P->H20>CNC)

H20> P-> CND)

P-> CN-> H20

E) none of these

3. As long as the disorder of the surroundings is increasing, a process will be ————-

4. The hydrogen sulfate or bisulfate ion HSO4- can act as either an acid or a base in water solution. In which of the following equations does HSO4- act as an acid?

A) HSO4- +H20 -t SO4~ + H30+

B) HSO4- + H20-t H2S04 +OH-

C) HS04- + H30+ -t S03 + 2H20

D) HS04- +OH–t H2S04 + 02

E) none of these

5. Delta Ho is zero for a chemical reaction at constant temperature

6. The heat of vaporization for 1.0 mole of water at 100°C and 1.0 atm is 40.6 kJ/mol. Calculate DeltaS for the process H20(1) -t H20(g) at 100°C.

A) 109 JIK mol   B) -406 JIK mol  C) -109 JIK mol  D) 406 JIK molE) none of these

7. What is the pH of a 0.45MKCI solution?

A) 1.4 B) 10.5 C) 9.2 D) 4.5 E) 7.0

8. For weak acid, HX, K = 1.0 x 10-6. Calculate the pH of a 0.10 M solution of HX.

A) 2.50 B) 3.00 C) a -6.00     D) 3.50     E) none of these

Use the following to answer question 9:

   Substance X has a heat of vaporization of 55.4 kJ/mol at its normal boiling point (423°C). For the process X (l)-t X(g) at 1 atm and 423°C calculate the value of:

9) ‘ A) -103 JIK·mol B) 79.6IIK·mol C) 103 JIK·mol D) -79.6IIK·mol   E) 0

10. The third law of thermodynamics states

A) the entropy of the universe is increasing

B) the entropy of the universe is constant

C) the entropy is zero at 0 K for a perfect crystal.

D) the absolute entropy of a substance decreases with increasing temperature.

E) the entropy of the universe equals the sum of the entropy of system and surroundings.

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