2.  What is a Lewis base?   a) an H⁺¹ acceptor   b) H₃O⁺¹ in H₂O   c)  OH^-1   d)  an electron pair provider

 3. What is the concentration of [H⁺¹] in 0.05 M H₂SO₄? a) 1 x 10^-14  b) 0.24  c) 1 x 10^-14/ 0.05    d) 0.10    d) .05

 4. The salt NaF reacts with water to produce: a)  H₂F      b)   H₃O⁺¹   c)  OH^-1   b) NaCl

 5. Which one of the following is a is strong acid?    a) HNO₃     b)  HClO  c) H₂SO₃  d) H₂CO₃

 6. In water the F^-1 ion will produce an acidic solution.  a) true b) false

 7. A species that can accept an H⁺¹ from another species is a(an): a) Arrhenius acid b)  soft acid    c) Lewis base
    d) Bronsted base

 8. What is the conjugate acid of the Bronsted base, OH^-1: a) O⁺¹  b) O^-2 c) H₂O  d) H₃O⁺¹

 9. A pH of 7 will be: a) acidic b) basic c) neutral

10. A 1.0 M strong base will have a pH of approximately  a) 14   b) 10   c) 7   d) 0    e)   -1

11. What happens to [OH^-1] when NaF is added to a water?  a) increases  b) decreases  c) stay the same

12. What is the numerical value of K_w? a) 14  b) 1 x 10^-14  c)  1 x 10^-7   d)  5.6 x 10^-10

13. The pupose of a buffer is:  a) make a  solution acidic b)  affect the solubility of a slightly solube salt
       c) keep pH fairly constant pH    d) cause a formation reaction

14. The conjugate of a strong Bronsted base is:  a) weak Bronsted base  b) weak Bronsted acid c)  strong  Bronsted base
      d) strong Bronsted acid

15. Solubility product calculations are used for: a) weak acid  b) slightly soluble ionic compoundt  
       c) salt of a weak acid  d) formation reaction
 
Questions 3, 4, 5, & 6  refer to the following equation

2 ICl₃ (g)    ◄══► I₂ (g)  +  3 Cl₂ (g)     ΔH = -45 kJ

16.  Adding ICl₃ to the system at equilibrium will: a) shift the system to the left  b) shift the system to the right 
       c) not affect the system  d) can't tell from information given

17. Adding a catalyst to the system at equilibrium will: a) shift the system to the left  b) shift the system to the right  
       c) not affect the system  d) can't tell from information given

18.  Increasing the temperature of the system at equili- brium will:  a) shift the system to the left  
       b) shift the system to the right  c) not affect the system     d) can't tell from information given

19. Increasing the pressure on the system at equilibrium will:  a) shift the system to the left  
      b) shift the system to the right  c) not affect the system     d) can't tell from information given

20. Define pH.

21. If the [OH^-1] of a solution is 6.4 x 10^-9, what is the [H₃O⁺¹]?

        is this solution acidic or basic?  ______

22. Balance the chemical equation for the ionization of the Bronsted base, NH₃ in water

23. Define the following terms:
       a) solubility product
       b) auto ionization
       c) K_w expression (not the value of it)

24. Calculate pH, pOH, [H₃O⁺¹], [OH^-1] of 0.08 M ammonium hydroxide, NH₄OH , solution?  K_b of NH₄OH  = 1.8 x 10^-5

25.  Given:  a 0.45 M NH₄Cl,    K_b of the base NH₄OH(NH₃ aq)  is 1.8 x 10^-5

    a) Give the chemical reaction of NH₄⁺¹ in water.

    b) give the K_a or K_b expression for the reaction in part A.

    c) Calculate the pH, of the solution

26.  Write the chemical equation for the ionization of water.

      Write the expression for K_w

27 Identify the titration curves as weak acid, strong acid, weak base, strong base with either strong base or strong acid
     added to the orginal soltuion
 

               ______________________________    ___________________________________

28. Write equilibrium constant expressions for the following molecular equilibrium:
                     a)   N₂ (g)   +    3   H₂ (g)     ◄══►  2  NH₃  (g)
                     b)  CaCO₃  (s)  ◄══►  CaO (s)    +    CO₂  (g)
29. What is one of the two general methods of preparing a buffer?

30. A buffer is prepared by making a solution containing 0.66 M NaF and 0.22 M HF.  Give the K_a
      expression for HF, then calculate pH of the buffer solution. K_a of the acid HF is 7.2 x 10^-4

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