Exercises
37.Calculate the pH of a 0.010 M solution of iodic acid(HIO3, Ka=0.17).
47.Calculate the percent dissociation of the acid in each of the following solutions.
   a. 0.50 M acetic acid              1.8*10(-5)
   b. 0.050 M acetic acid
   c. 0.0050 M acetic acid
   d. Use Le Chatelier’s principle to explain why percent dissociation increases as the concentration of a weak acid decreases.
   e. Even though the percent dissociation increases from solutions a to c, the [H+] decreases . Explain.
53.Arsenic acid (H3AsO4)is a triprotic acid with Ka1 = 5 X 10-3, Ka2 = 8X10-8, Ka3 = 8X10-10. Calaulate [H+], [OH-], [H3AsO4], [H2AsO4-], [ HAsO42-], and [AsO43-] in a 0.20 Marsenic acid solution.
61.Calculate the pH of the following solutions.
   a. 0.10 M NaOH
   b. 1.0X10-10 M NaOH
   c. 2.0 M NaOH


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