1. ACIDS AND BASES www.lab-initio.com

2. Ga Standards

3. Properties of Acids  Acids are proton (hydrogen ion, H + ) donors  Acids have a pH lower than 7  Acids taste sour  Acids effect indicators  Blue litmus turns red  Methyl orange turns red  Acids react with active metals, producing H 2  Acids react with carbonates  Acids neutralize bases

4. Acids are Proton (H + ion) Donors Strong acids are assumed to be 100% ionized in solution (good H + donors). Weak acids are usually less than 5% ionized in solution (poor H + donors). HClH 2 SO 4 HNO 3 H 3 PO 4 HC2H3O2HC2H3O2 Organic acids

5. Acids Have a pH less than 7

6. Acids Taste Sour  Citric acid in citrus fruit  Malic acid in sour apples  Lactic acid in sour milk and sore muscles  Butyric acid in rancid butter Organic acids are weak acids. Some are used as flavoring agents in food.

7. Organic Acids Organic acids all contain the “carboxyl” group, sometimes several of them. The carboxyl group is a poor proton donor, so ALL organic acids are weak acids.

8. Acids Effect Indicators Blue litmus paper turns red in contact with an acid. Methyl orange turns red with addition of an acid

9. Acids React with Active Metals Acids react with active metals to form salts and hydrogen gas. Mg + 2HCl  MgCl 2 + H 2 (g) Zn + 2HCl  ZnCl 2 + H 2 (g) Mg + H 2 SO 4  MgSO 4 + H 2 (g)

10. Acids React with Carbonates 2HC 2 H 3 O 2 + Na 2 CO 3 2 NaC 2 H 3 O 2 + H 2 O + CO 2

11. Effects of Acid Rain on Marble (calcium carbonate) George Washington: BEFORE George Washington: AFTER

12. Acids Neutralize Bases HCl + NaOH  NaCl + H 2 O Neutralization reactions ALWAYS produce a salt and water. H 2 SO 4 + 2NaOH  Na 2 SO 4 + 2H 2 O 2HNO 3 + Mg(OH) 2  Mg(NO 3 ) 2 + 2H 2 O

13. Properties of Bases  Bases are proton (hydrogen ion, H + ) acceptors  Bases have a pH greater than 7  Bases taste bitter  Bases effect indicators  Red litmus turns blue  Phenolphthalein turns purple  Solutions of bases feel slippery  Bases neutralize acids

14. Bases are Proton (H + ion) Acceptors  Sodium hydroxide (lye), NaOH  Potassium hydroxide, KOH  Magnesium hydroxide, Mg(OH) 2  Calcium hydroxide (lime), Ca(OH) 2 OH - (hydroxide) in base combines with H + in acids to form water H + + OH -  H 2 O

15. Bases have a pH greater than 7

16. Bases Effect Indicators Red litmus paper turns blue in contact with a base. Phenolphthalein turns bright pink in a base.

17. Bases Neutralize Acids Milk of Magnesia contains magnesium hydroxide, Mg(OH) 2, which neutralizes stomach acid, HCl. 2 HCl + Mg(OH) 2 MgCl 2 + 2 H 2 O

18. pH Calculations Soren Sorensen SPECIAL NOTE: In pH chemistry, H + is often used as an abbreviation for H 3 O + ! ! ! ! ! ! ! ! !

19. pH Scale

20. Self-Ionization of Water H 2 O + H 2 O  H 3 O + + OH - Though pure water is considered a non-conductor, there is a slight, but measurable conductivity due to “self- ionization”

21. K w – Ionization Constant for Water In pure water at 25  C: [H 3 O + ] = 1 x 10 -7 mol/L [OH - ] = 1 x 10 -7 mol/L K w is a constant at 25  C: Kw = [H 3 O + ][OH - ] Kw = (1 x 10 -7 )(1 x 10 -7 ) = 1 x 10 -14

22. Calculating pH, pOH pH = -log 10 (H 3 O + ) pOH = -log 10 (OH - ) Relationship between pH and pOH pH + pOH = 14 Finding [H 3 O + ], [OH - ] from pH, pOH [H 3 O + ] = 10 -pH [OH - ] = 10 -pOH

23. pH + pOH = 14