1 / 22

Aqueous Reactions and Solution Stoichiometry

Aqueous Reactions and Solution Stoichiometry. Know the symbols. g s l aq c. What is the difference between a “liquid solution” and an “aqueous solution” ?. Which of the following would be an electrolytic or non-electrolytic solution ?. NO NaCl PCl 3 CO 2 MgSO 4.

taylor
Download Presentation

Aqueous Reactions and Solution Stoichiometry

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. Aqueous Reactions and Solution Stoichiometry

  2. Know the symbols • g • s • l • aq • c

  3. What is the difference between a “liquid solution” and an “aqueous solution” ?

  4. Which of the following would be an electrolytic or non-electrolytic solution ? • NO • NaCl • PCl3 • CO2 • MgSO4

  5. Weak vs Strong Electrolytes • Use a single arrow to show a reaction with a strong electrolyte. • Use a double arrow to show a reaction with a weak electrolyte.

  6. Precipitation Reactions • Precipitation reactions are reactions that result in the formation of an insoluble product. • Make sure to use an “s” to designate the solid that precipitates.

  7. Solubility Rules • You must memorize the solubility rules for the AP exam and for a quiz in class.

  8. Ionic Equations • You need to know the difference between the following types of equations: • Molecular equations • Complete ion equations • Net ionic equations • What is a spectator ion?

  9. How to write a “Net Ionic Equation” • Write a balanced molecular equation. • Rewrite the equation showing all strong electrolytes that dissociate (or ionize) in solution. • Cancel out spectator ions.

  10. Acid Base Reactions • You need to memorize the list of strong acids and bases. • Acids: • HCl • HBr • HI • HClO3 chloric acid • HClO4 perchloric acid • HNO3 nitric acid • H2SO4 sulfuric acid

  11. Bases: • Group 1A metal hydroxides (LiOH, NaOH, KOH, RbOH, CsOH) • Heavy group 2A metal hydroxides • Ca(OH)2 , Sr(OH)2 , Ba(OH)2

  12. What do you get when you mix an acid and a base? • Any thoughts? • A neutralization reaction • Can you explain how the water is produced in a neutralization reaction?

  13. Oxidation-Reduction Reactions • OIL oxidation is loss of electrons • RIG reduction is gain of electrons • See the textbook for the rules for assigning oxidation numbers.

  14. Activity Series • You can use the activity series to determine if some reactions involving metals will occur. • An activity series is a list of metals arranged in order of decreasing ease of oxidation. • See the textbook for the activity series diagram.

  15. You will need to memorize the activity series for the AP exam. • Look at the AP Reference packet. Take a good look at the Standard Reduction Potential chart.

  16. Molarity moles of solute Molarity = liters of solution Molarity is another way to express concentration.

  17. Molality moles of solute Molality = kilograms of solvent Molality is another way to express concentration.

  18. Dilution MiVi = MfVf i is the initial concentration f is the final concentration

  19. Titrations • Use titrations to determine the concentration of a solution. • The point in a titration when stoichiometrically amounts are brought together is called the equivalence point. • You titrate an unknown solution with a standard solution. Use an indicator to show when the equivalence point has been reached. • The color change during a titration signals the endpoint which is very close to the equivalence point.

  20. Titration Calculations • If you are given a volume and molarity for a substance, start the calculation with that. • Convert to moles of what you know • then use the molar ratios to convert to moles of the unknown substance • Finally, use the volume of the unknown substance to convert to molarity.

  21. Titrations • You can use the dilution equation to solve titration problems, as long as the molar ratio is 1 to 1.

  22. Problems to Try • 5, 6, 7, 9, 10, 11, 13, 16, 17, 18, 21, 26, 27, 28, 35, 37, 39, 41, 43, 46, 51, 53, 54, 56, 59, 60, 63, 65, 66, 67, 69, 71, 73, 76, 78, 81, 89, 90

More Related