1602 ACID BASE EQUILIBRIA PART 2

    16.5 (17pts)

  1. What are strong acids and bases in aqueous solutions?
  2. What are the seven most common strong monoprotic acids and the one diprotic acid?
  3. Write the eqautuon for nitric acid and water.
  4. What is used interchangeably to represent the hydrated proton in water?
  5. How do you calculate the pH of a strong monoprotic acid?
  6. What are the strong bases?
  7. Write out sample exercise 16.9.
  8. Explain what happens when a solution formed by dissolving 0.010 mol of Na2O(s) in enough water to form 1.0 L solution.
  9. problems 9pts



16.6 (20pts)

  1. What is the general equation for a weak acid?
  2. Why is H2O not in the eqaution?
  3. What are two different ways to write the equilibrium-constant expression?
  4. What does Ka signify?
  5. The magnitude of Ka indicates the __________________________________________: The larger the value of Ka, the __________________________. For most weak acids, Ka values range from ____________ to ____________.
  6. Follow sample exercise 16.10, and complete this problem. A student prepared a 0.10 M solution of formic acid and found its pH at to be 2.38. Calculate Ka for formic acid at this temperature.
  7. What is percent ionization?
  8. What is percent ionization of a 0.035 M solution of HNO2 which contains 3.7x10-3 M of H+?
  9. On page 670, write out the steps for calculating Ka from pH.
  10. In the example, write out how the % ionization was calculated.
  11. As a general rule, if x is more than about ______% of the initial concentration value, it is better to use the quadratic formula. You should always check the validity of any simplifying assumptions after you have finished solving a problem.
  12. Higher the pH the ______ acidic.
  13. The pH of 0.30M Acetic acid is _________. The pH of 0.30M HCL is ___________.
  14. Doubling the concentration fo a weak acid ____________ double the concentration of H+ ions.
  15. Calculate the percent ionization of a) 0.10M HF and b) 0.010M HF (hint page 673).
  16. What is a polyprotic acid?
  17. Using H2SO3 as an example, show the two equilibrium equations and their Ka values.
  18. Why would Ka2 always be less than Ka1?
  19. It is always easier to remove the _______ proton of a polyprotic acid than the _______ one.
  20. Write out what occurs for dissociation with sulfuric acid.

16.6 PROBLEMS (18pts)








 

 

 

 

 

 
 

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