1 / 15

Chapter 14 Acids and Bases

Chapter 14 Acids and Bases. Acid-Base Reactions. 14-3. 14-3 Learning Targets. Describe a conjugate acid, a conjugate base, and an amphoteric compound Explain the process of neutralization and identify examples. Bronsted- Lowry Acids and Bases.

hweaver
Télécharger la présentation

Chapter 14 Acids and Bases

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 14 Acids and Bases

  2. Acid-Base Reactions 14-3

  3. 14-3 Learning Targets • Describe a conjugate acid, a conjugate base, and an amphoteric compound • Explain the process of neutralization and identify examples

  4. Bronsted- Lowry Acids and Bases • Bronsted-Lowry Acid- molecule or ion that is a proton donor • HCl + NH3→ NH4+ + Cl- • HCl is acid, ammonia is base • Bronsted-Lowry Base- molecule or ion proton acceptor • Hydroxide ions is the acceptor of ionic bases, NOT the ionic compound itself • Bronsted-Lowry Acid-Base reaction- reaction where protons are transferred from the acid to the base

  5. Bronsted-Lowry Acid-Base reaction- reaction where protons are transferred from the acid to the base • involve two acid-base pairs, known a conjugate acid-base pairs.

  6. Conjugate Acids and Bases • Conjugate Base- the species that remains after an acid has given up a proton • H3PO4(aq) + H2O (l) ↔ H3O+ (aq) + H2PO4– (aq) acid conjugate base • The stronger the acid the weaker its conjugate base • Conjugate acid- the species that is formed when a base gains a proton • H3PO4(aq) + H2O (l) ↔ H3O+ (aq) + H2PO4– (aq) • base conjugate acid • The stronger a base, the weaker its conjugate acid

  7. Conjugate Acids and Bases

  8. Proton transfer reactions favor the production of the weaker acid and the weaker base • HClO4 (aq) + H2O(l) → H3O+ (aq) + ClO- (aq) stronger acid stronger base weaker acid weaker base • The reaction to the right is more favorable • C2H4O2 (aq) + H2O(l) → H3O+ (aq) + C2H3O2 - (aq) weaker acid weaker base stronger acid stronger base • The reaction to the left is more favorable

  9. Amphoteric Compounds • Amphoteric- any species that can react as either an acid or a base • Water as a base • H3PO4(aq) + H2O (l) ↔ H3O+ (aq) + H2PO4– (aq) • Water as an acid • NH3 (g) + H2O (l) ↔NH4+ (aq) + OH- (aq)

  10. OH- in a molecule • Hydroxyl group • OH group can be acidic or amphoteric • As the number of oxygens that are bonded around the atom with the –OH group increased the acidity of the compound increases • Oxygens pull electron density away from the hydrogen, making it appear more positive ( attractive to water and other bases) • Increasing acidity HClO, HClO2, HClO3, HClO4

  11. Neutralization Reactions • Neutralization- reaction of hydronium ions and hydroxide ions to form water molecules ( and a salt) • Neutralization Reaction • KOH (aq) + HNO3 (aq) → KNO3 (aq) + H2O (l) • Step 1: Dissociation of a base in water • KOH (aq) →K+ (aq) + OH- • Step 2: Acid donate a proton to water • HNO3 (aq) + H2O (l) →H3O+ (aq) + NO3- (aq)

  12. Complete Ionic equation • K+ (aq) + OH – (aq) + H3O+ (aq) +NO3 -(aq) → K + (aq) +NO3-(aq) + 2H2O (l) • Net ionic equation (eliminate spectator ions) • H3O+ (aq) + OH – (aq) →2H2O (l)

  13. Strong acid + Strong base= Neutral salt • Strong acid + Weak base = Acidic salt • Weak acid + Strong base = Basic salt

  14. Acid Rain • Nonmetallic oxides enter the atmosphere as a result of coal burning, auto exhaust, and air pollution • SO2 SO3 CO2 NO NO2 • Nonmetallic oxides combine with water to form oxyacids • SO3 (g) + H2O (l) →H2SO4 (aq) • Acid rain reacts with marble (metamorphic carbonate) • CaCO3 (s) + 2H3O+ (aq) → Ca 2+ (aq) + CO2 (g) + 3H2O (l)

More Related