Classwork – Reactions in Aqueous Solutions I (Precipitation Reactions)

  1. List the four common driving forces that make reactions go forward.
  2. Provide an example for each of the driving forces.
  3. Describe what happens in a precipitation reaction.
  4. Sketch a molecular-level representation that demonstrates how/why an electrolyte allows electric current to flow through.
  5. Describe what is meant by “strong electrolyte.”
  6. Write the balanced equation that shows barium nitrate dissolving in water.
  7. Write the correct formula for sodium sulfate, and write a balanced equation that would show sodium sulfate dissolving in water.
  8. Sketch a molecular-level representation that shows both potassium chromate and one that shows barium nitrate each dissolved in water in their ion forms.
  9. List all four possible combinations of cation and anion that might form when potassium chromate reacts with barium nitrate.
  10. Sketch a molecular-level representation that shows all the ions in solution together before potassium chromate reacts with barium nitrate and one that shows them after reaction has taken place.
  11. How do we know that neither potassium chromate nor barium nitrate was the solid that formed in the reaction in question #10 above?
  12. Distinguish between a soluble solid and an insoluble (slightly soluble) solid.
  13. Use your solubility rules to identify the following salts as either soluble or insoluble:
  14. sodium nitrate
  15. sodium sulfate
  16. potassium chloride
  17. silver chloride
  18. lead sulfate
  19. sodium hydroxide
  20. lead hydroxide
  21. When silver nitrate reacts with sodium chloride a white solid precipitate forms. Use your solubility rules to identify the solid. Write a balanced chemical equation for the reaction.
  22. Predict whether a solid will form when the following pairs of solutions are mixed. If so, identify the solid and write the balanced equation for the reaction:
  23. barium nitrate and sodium chloride
  24. sodium sulfide and copper (II) nitrate
  25. ammonium chloride and lead (II) nitrate
  26. Distinguish between molecular equation and net ionic equation.
  27. Explain the term spectator ion.
  28. A solution of lead (II) nitrate is reacted with a solution of potassium iodide. Write a molecular equation, complete ionic equation, and net ionic equation for this reaction.
  29. According to the solubility rules, which ions are generally spectator ions?
  30. What is the advantage of writing net ionic equations for chemical reactions?