1. Acids Lesson 1 Acid and Base Properties

2. Taste sour Change litmus paper red React with metals such as Mg and Zn to make H 2 Are electrolytes that conduct electricity Neutralize bases Properties of Acids

3. Taste bitter Change litmus paper blue Feel slippery Are electrolytes that conduct electricity Neutralize acids Properties of Bases

4. Arrhenius acid HCl  Arrhenius base NaOH  Na + + OH - H + + Cl - produces H + in solutionChemistry 11 produces OH - in solutionChemistry 11

5. H+H+ Bronsted Acid H+H+ HCl + H 2 O  Bronsted Base NH 3 + H 2 O ⇄ A proton donor A proton acceptor Chemistry 12 H 3 O + + Cl - NH 4 + + OH - weak strong

6. H+H+ H+H+ Write a Bronsted reaction for the base HCO 3 - base acid base HCO 3 - ⇄ H 2 CO 3 + OH - + H 2 O weak Conjugate acid base pairs differ by one proton H + HCO 3 - and H 2 CO 3 H 2 O and OH -

7. 5. H + is the same as H 3 O + 4. Bronsted acids donate a proton to water to form H 3 O + 3. Arrhenius acids dissociate in water to form H + 2. Bronsted bases accept a proton from water to produce OH - 1. Arrhenius bases dissociate in water to produce OH - Note

8. H + is another way to show H 3 O +. Hydronium ion H3O+H3O+ H + + H 2 O ⇋ + H+H+ H2OH2O

9. NH 4 + NH 3 Fe(H 2 O) 6 3+ OH - HCO 3 - HPO 4 2- PO 4 3- HPO 4 2- H 2 PO 4 - H 2 CO 3 H2OH2O One more H + 1 less H + Conjugate BaseConjugate Acid C 6 H 5 COOHC 6 H 5 COO - C 6 H 5 OHC6H5O-C6H5O- Fe(H 2 O) 5 (OH) 2+ Look on page 6

10. Strong Acids Weak Acids

11. HCl + H 2 O  H 3 O + + Cl - Use a “  ” and not “ ⇄ ” Have very large Ka’s. Produce large amounts of H 3 O +. Are good conductors. Completely ionize in water Left side Acid Chart top six Strong Acids

12. Weak Acids Left side of the Acid Chart below the top six. Do not completely ionize in water. Are poor conductors. Produce small amounts of H 3 O +. Have small Ka’s. Use a “ ⇄ ” and not “  ” HF + H 2 O ⇄ H 3 O + + F - Ka=[H 3 O + ][F - ] =3.5 x 10 -4 from page 6 [HF] Water is not included because it is a pure liquid! Its concentration is constant !

13. You can also write: HF ⇌ H + + F - Ka= [H + ][F - ] =3.5 x 10 -4 [HF]

14. HF + OH -  F - + H 2 O (l) HF + K + + OH -  K + + F - + H 2 O (l) HF + KOH  KF+H 2 O (l) Do not break up weak acids or bases! H + + OH -  H 2 O (l) H + + Cl - + Na + + OH -  Na + + Cl - + H 2 O (l) HCl + NaOH  NaCl+H 2 O (l) Writing Ionic Equations: Formula, Complete, and Net. HF is a weak acid