2. Acids, Bases, & Salts

3. What is an ACID? pH less than 7

4. What is an ACID? pH less than 7 Neutralizes bases

5. What is an ACID? pH less than 7 Neutralizes bases Forms H + ions in solution H+H+ H+H+ H+H+ H+H+ H+H+ H+H+ H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O

6. What is an ACID? pH less than 7 Neutralizes bases Forms H + ions in solution Corrosive-reacts with metals

7. What is an ACID? pH less than 7 Neutralizes bases Forms H + ions in solution Corrosive-reacts with most metals to form hydrogen gas Good conductors of electricity

8. What is an ACID? pH less than 7 Neutralizes bases Forms H + ions in solution Corrosive-reacts with most metals to form hydrogen gas Good conductors of electricity Tastes Sour

9. Acids Generate Hydronium Ions HNO 3 + H 2 O  H + + H 2 O + NO3  H 3 O + + NO 3

10. Weak vs. Strong Acids Weak Acids do not ionize completely: Acetic, Boric, Nitrous, Phosphoric, Sulfurous Strong Acids ionize completely: Hydrochloric, Nitric; Sulfuric, Hydriodic

11. Common Acids HCl- hydrochloric- stomach acid H 2 SO 4 - sulfuric acid - car batteries HNO 3 – nitric acid - explosives HC 2 H 3 O 2 - acetic acid - vinegar H 2 CO 3 - carbonic acid – sodas H 3 PO 4 - phosphoric acid -flavorings

12. What is a BASE? pH greater than 7

13. What is a BASE? pH greater than 7 Feels slippery

14. What is a BASE? pH greater than 7 Feels slippery Tastes Bitter

15. What is a BASE? pH greater than 7 Feels slippery Bitter Taste Usually forms OH - ions in solution OH - H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O H2OH2O

16. What is a BASE? pH greater than 7 Feels slippery Tastes Bitter Usually forms OH - ions in solution Neutralizes acids

17. What is a BASE? pH greater than 7 Feels slippery Tastes Bitter Usually forms OH - ions in solution Neutralizes acids Conducts Electricity

18. Common Bases NaOH- sodium hydroxide (LYE) soaps, drain cleaner Mg (OH) 2 - magnesium hydroxide - antacids Al(OH) 3 - aluminum hydroxide - antacids, deodorants NH 4 OH - ammonium hydroxide - “ammonia”

19. pH of Common Substances Timberlake, Chemistry 7 th Edition, page 335 HCl Gastric Juice Lemon Juice Vinegar

20. pH of Common Substances Timberlake, Chemistry 7 th Edition, page 335 Orange Soda Apple Tomato Coffee Soil Bread Potato Urine Milk

21. pH of Common Substances Timberlake, Chemistry 7 th Edition, page 335 Pure Water

22. pH of Common Substances Timberlake, Chemistry 7 th Edition, page 335 Drinking Water Blood Detergents Bile Sea Water

23. pH of Common Substances Timberlake, Chemistry 7 th Edition, page 335 Milk of Magnesia Ammonia Bleach Lye (NaOH)

24. pH paper pH paper changes color to indicate a specific pH value.

25. Buffers A buffer is a solution that resists changes in pH when small amounts of acids and bases are added.

26. Situations in which pH is controlled “Heartburn” Planting vegetables and flowers Fish Tanks and Ponds Blood Swimming pools

27. Acids and Bases in Solution HCl + H 2 0  H 3 O + + Cl - (more hydronium ions, more acidic)

28. Acids and Bases in Solution HCl + H 2 0  H 3 O + + Cl - (more hydronium ions, more acidic) NaOH in water  Na + + OH - (more hydroxide ions, more basic)

29. Acids and Bases in Solution HCl + H 2 0  H 3 O + + Cl - (more hydronium ions, more acidic) NaOH in water  Na + + OH - (more hydroxide ions, more basic) HCl + NaOH  NaCl + HOH Acid + Base yields type of salt and water

30. Neutralization Reaction reaction of an acid with a base to produce salt and water. Example H 2 SO4 + NaOH  NaHSO 4 + H 2 O

31. Acid Rain Pollution in the air (sulfur dioxide, carbon dioxide, nitrogen dioxide) combines with water to form various acids..

33. Rapid changes in pH can kill organisms in lakes and streams. can kill plants and create sinkholes

36. What is a SALT? Composed of the negative ion of an acid and the positive ion of a base. One of the products of a Neutralization Reaction Examples: KCl, NaCl, MgSO 4, Na 3 PO 4

37. Acids, Bases, and Salts The End