1 / 11

Chapter 4:Aqueous Reactions and Solution Stoichiometry

Chapter 4:Aqueous Reactions and Solution Stoichiometry. 4.1 Aqueous Solutions. Electrolytes - ionic solutions that conduct a current. ZAP. Nonelectrolytes - molecular compounds (most covalent) Strong electrolytes - strong acids, strong bases, and salts

lorant
Download Presentation

Chapter 4: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. Chapter 4:Aqueous Reactions and Solution Stoichiometry

  2. 4.1 Aqueous Solutions • Electrolytes- ionic solutions that conduct a current. ZAP. • Nonelectrolytes- molecular compounds (most covalent) • Strong electrolytes- strong acids, strong bases, and salts • Weak electrolytes- weak acids and weak bases

  3. 4.3 Reactions A. Double Displacement AB + CD  AD + CB • Precipitate • Solubility rules (p. 125) • Neutralization • Acid + base  salt + H2O • Hydrolysis • Salt + water  acid + base B. Single Displacement Element + compound  element + compound • Activity Series p141 • Metal • Nonmetals

  4. Combustion • Complete • Comp + O2 CO2 + H2O • Incomplete • Comp + O2 CO + H2O • Synthesis ( A + B  C) • Element + element  compound • Acid anhydride + water  acid • Base anhydride + water  base • AA + BA  salt • Decomposition (A  B + C) • Acid  AA + water • Base  BA + water • 2KClO3  2KCl + 3O2

  5. Carbonates  CO2 + metal oxides (CaCO3  CO2 + CaO) • H2CO3  H2O + CO2 • H2SO3  H2O + SO2 • NH4OH  H2O + NH3 • Binary Compound  element + element • 2H2O2  2H2O + O2 • Red – ox (oxidation reduction)these totally suck and will come back around chapter 20. • Oxidation • Gain in oxidation number • Loses electrons • Is a reducing agent • Reduction • Reduced in oxidation number • Gains electrons • Is an oxidizing agent • Net Ionic Equations • Spectator Ions LEO - GER

  6. 4.5 Concentrations of Solutions Sample 4.11 How many grams of Na2SO4 are required to make 0.350 liter of 0.500 M Na2SO4?

  7. 4.5 Concentrations of Solutions Sample 4.11 How many grams of Na2SO4 are required to make 0.350 liter of 0.500 M Na2SO4?

  8. Dilutions Sample 4.12

  9. 4.6 Solution Stoichiometry • Sample 4.13 • Titrations (don’t forget your magic! Except you have no idea what I’m talking about, this being only chapter 4. Aww, I bet you still think you’re going to pass the AP Exam, don’t you?) • Standard solution – known concentration • Equivalence point – Stoichiometry equivalent • Acid-base-indicators – solution that is one color in acid solution and another in basic solution • End point- color change MOLES OF ACID = MOLES OF BASE @ EQUIVALENCE POINT

  10. Sample 4.15

  11. THE END This PowerPoint was made by the dutiful David Drewry. Lilly made the soul crushing commentary.

More Related