1 / 20

CHEMISTRY 161 Chapter 4

CHEMISTRY 161 Chapter 4. REVISION. solution, solvent, and solute 2. experimental definition of strong/weak/non-electrolyte 3. dissociation and hydration of solute in solvent (solutions conduct electricity) 4. precipitation reaction (molecular equation, ionic equation, spectator ions).

quentin-bonner
Download Presentation

CHEMISTRY 161 Chapter 4

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. CHEMISTRY 161 Chapter 4

  2. REVISION • solution, solvent, and solute • 2. experimental definition of strong/weak/non-electrolyte • 3. dissociation and hydration of solute in solvent • (solutions conduct electricity) • 4. precipitation reaction • (molecular equation, ionic equation, spectator ions)

  3. CHEMICAL REACTIONS • properties of solutions • 2. reactions in solutions • a) precipitation reactions • b) acid-base reactions (proton transfer) • c)redox reactions (electron transfer)

  4. 2.2. ACIDS AND BASES ACIDS HAc → H+ (aq) + Ac- (aq) HCl (g) →H+ (aq) + Cl- (aq) BASES MOH → M+ (aq) + OH- (aq) Arrhenius (1883) NaOH (s) →Na+ (aq) + OH- (aq)

  5. ACIDS • acids have a sour taste • vinegar – acetic acid • lemons – citric acid 2. acids react with some metals to form hydrogen 2 HCl(aq) + Mg(s) → MgCl2(aq) + H2(g) 3. acids react with carbonates to water and carbon dioxide 2 HCl(aq) + CaCO3(s) → CaCl2(aq) + [H2CO3] H2CO3 → H2O(l) + CO2(g)

  6. BASES • bases have a bitter taste 2. bases feel slippery soap 3. aqueous bases and acids conduct electricity

  7. ACIDS proton donors HAc → H+ (aq) + Ac- (aq) BASES proton acceptor B + H+ (aq) → BH+ (aq) Bronsted (1932)

  8. ≈ 10-15 m H+ ≈ 10-10 m Na+

  9. (aq) (l) (aq) (aq) acid base hydronium ion

  10. cation hydronium ion

  11. strong electrolyte HCl(aq) + H2O(l) → H3O+(aq) + Cl-(aq) HNO3(aq) + H2O(l) → H3O+(aq) + NO3-(aq) weak electrolyte CH3COOH(aq) + H2O(l) H3O+(aq) + CH3COO-(aq) NH3(aq) + H2O(l) NH4+ + OH- monoprotic acids

  12. CH3COOH(aq) + H2O(l) H3O+(aq) + CH3COO-(aq) NH3(aq) + H2O(l) NH4+(aq)+ OH-(aq) H2O(l) + H2O(l) H3O+(aq) + OH-(aq) water can be either an acid or a base

  13. monoprotic acids HF, HCl, HBr, HNO3, CH3COOH diprotic acid H2SO4→ H+(aq) + HSO4-(aq) HSO4-(aq) H+(aq) + SO42-(aq) triprotic acid H3PO4 H+(aq) + H2PO4-(aq) H2PO4-(aq) H+(aq) + HPO42-(aq) HPO42-(aq) H+(aq) + PO43-(aq)

  14. Acids in the Solar System Europa H2SO4(s) Venus H2SO4(g)

  15. Acids in the Interstellar Medium

  16. NH3, H2O, H2S CH3COOH HCOOH HF, HCl Orion

  17. ACID-BASE REACTION acid + base→ salt + water (neutralization reaction) HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) molecular equation – ionic equation – spectator ions

  18. SUMMARY • acids and bases • 1.1. Arrhenius and Bronsted • 1.2. strong and weak acids and bases • 1.3 acids in extraterrestrial environments • 2. acid-base neutralization reactions

  19. Homework Chapter 4, p. 111-116 problems

More Related