AP Chemistry, Predicting Products:Sec. 8.14 – 8.16 Reading Guide

  1. What are the two possible products when a solid dissolves?
  2. How can you tell whether a solid will most likely produce molecules or ions when it dissolves?
  3. Compare and Contrast strong electrolytes, weak electrolytes, and nonelectrolytes.
  4. Explain how the conductivity apparatus works and how the results would indicate what kind of electrolyte the solution is.
  5. Using a more sensitive tester for conductivity, why does the conductivity of a silver chloride solution increase as more silver chloride solid is added?
  6. What happens that eventually the amount of conductivity of a silver chloride solution stops increasing?
  7. What macroscopic observations should you be able to make about a beaker of water with silver chloride if it has reached the point where the conductivity stops increasing?
  8. What is the connection between the solubility of a substance, a saturated solution, and a precipitation reaction?
  9. Most of our level of chemistry will involve solids we term either soluble or insoluble, what concentration will probably separate those two categories?
  10. What four ions are always soluble (that is there are no exceptions)? Memorize these!
  11. For the groups of ions marked “insoluble”, what ions are exceptions to them all?
  12. Contrast condensed equations, ionic equations, and net ionic equations. Show an example of each.
  13. What are spectator ions, and what is necessary to classify an ion as such?
  14. What is the most difficult task of writing net ionic equations?
  15. What three types of substances are considered strong electrolytes?
  16. What are the strong acids and strong bases? Memorize these!
  17. Work exercise 8.4 (cover up the answers at first) and then check your work.

AP Chemistry, Predicting Products:Sec. 8.14 – 8.16 Reading Guide

  1. What are the two possible products when a solid dissolves?
  2. How can you tell whether a solid will most likely produce molecules or ions when it dissolves?
  3. Compare and Contrast strong electrolytes, weak electrolytes, and nonelectrolytes.
  4. Explain how the conductivity apparatus works and how the results would indicate what kind of electrolyte the solution is.
  5. Using a more sensitive tester for conductivity, why does the conductivity of a silver chloride solution increase as more silver chloride solid is added?
  6. What happens that eventually the amount of conductivity of a silver chloride solution stops increasing?
  7. What macroscopic observations should you be able to make about a beaker of water with silver chloride if it has reached the point where the conductivity stops increasing?
  8. What is the connection between the solubility of a substance, a saturated solution, and a precipitation reaction?
  9. Most of our level of chemistry will involve solids we term either soluble or insoluble, what concentration will probably separate those two categories?
  10. What four ions are always soluble (that is there are no exceptions)? Memorize these!
  11. For the groups of ions marked “insoluble”, what ions are exceptions to them all?
  12. Contrast condensed equations, ionic equations, and net ionic equations. Show an example of each.
  13. What are spectator ions, and what is necessary to classify an ion as such?
  14. What is the most difficult task of writing net ionic equations?
  15. What three types of substances are considered strong electrolytes?
  16. What are the strong acids and strong bases? Memorize these!
  17. Work exercise 8.4 (cover up the answers at first) and then check your work.