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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.

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Chapter 14 Acids and Bases

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  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)

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