1. I. Introduction to Acids & Bases (p. 453 - 473) Ch. 15 & 16 - Acids & Bases

3. A. Properties electrolytes  electrolytes electrolytes  electrolytes turn litmus red turn litmus red sour taste sour taste react with metals to form H 2 gas react with metals to form H 2 gas slippery feel slippery feel turn litmus blue turn litmus blue bitter taste bitter taste ChemASAP vinegar, milk, soda, apples, citrus fruits vinegar, milk, soda, apples, citrus fruits ammonia, lye, antacid, baking soda ammonia, lye, antacid, baking soda

4. SOME COMMON INDUSTRIAL ACIDS Sulfuric acid Sulfuric acid Most commonly produced industrial chemical Most commonly produced industrial chemical Uses: petroleum refining, metallurgy, manufacturing fertilizer, production of metals, paper, paint, dyes, detergents, and used in automobile batteries Uses: petroleum refining, metallurgy, manufacturing fertilizer, production of metals, paper, paint, dyes, detergents, and used in automobile batteries Effective dehydration agent Effective dehydration agent

5. SOME COMMON INDUSTRIAL ACIDS Nitric acid Nitric acid Pure nitric acid is a volatile, unstable liquid that is rarely used in industry or labs. Pure nitric acid is a volatile, unstable liquid that is rarely used in industry or labs. Strong odor, stains skin, and can cause serious burns Strong odor, stains skin, and can cause serious burns Used in making explosives, rubber, plastics, dyes and pharmaceuticals. Used in making explosives, rubber, plastics, dyes and pharmaceuticals.

6. SOME COMMON INDUSTRIAL ACIDS Phosphoric acid Phosphoric acid Essential element for plants and animals Essential element for plants and animals Used for manufacturing fertilizers and animal feed, diluted - flavoring agent in beverages, cleaning agent for dairy equipment, manufacture of detergents and ceramics. Used for manufacturing fertilizers and animal feed, diluted - flavoring agent in beverages, cleaning agent for dairy equipment, manufacture of detergents and ceramics.

7. SOME COMMON INDUSTRIAL ACIDS Hydrochloric acid Hydrochloric acid Produced by stomach and aids in digestion. Produced by stomach and aids in digestion. Used for pickling iron and steel, general cleaning agent, food processing, activation of oil wells, recovery of magnesium from sea water, production of other chemicals. Used for pickling iron and steel, general cleaning agent, food processing, activation of oil wells, recovery of magnesium from sea water, production of other chemicals. Dilute HCl, commonly known as muriatic acid, found in hardware stores and used for maintaining acidity in swimming pools and general cleaning of masonry. Dilute HCl, commonly known as muriatic acid, found in hardware stores and used for maintaining acidity in swimming pools and general cleaning of masonry.

8. SOME COMMON INDUSTRIAL ACIDS Acetic acid Acetic acid Clear, colorless, strong smell Clear, colorless, strong smell Concentrated form known as glacial acetic acid Concentrated form known as glacial acetic acid Used in synthesizing chemicals used in the manufacture of plastics, raw material in production of food supplements, fungicide. Used in synthesizing chemicals used in the manufacture of plastics, raw material in production of food supplements, fungicide.

9. B. Definitions Arrhenius - In aqueous solution… Arrhenius - In aqueous solution… HCl + H 2 O  H 3 O + + Cl – Acids form hydronium ions (H 3 O + ) Acids form hydronium ions (H 3 O + ) H HHHH H Cl OO – + acid

10. B. Definitions Arrhenius - In aqueous solution… Arrhenius - In aqueous solution… Bases form hydroxide ions (OH - ) Bases form hydroxide ions (OH - ) NH 3 + H 2 O  NH 4 + + OH - H H H H H H N NO O – + H H H H base

11. B. Definitions Brønsted-Lowry Brønsted-Lowry HCl + H 2 O  Cl – + H 3 O + Acids are proton (H + ) donors. Acids are proton (H + ) donors. Bases are proton (H + ) acceptors. Bases are proton (H + ) acceptors. conjugate acid conjugate base baseacid

12. B. Definitions H 2 O + HNO 3  H 3 O + + NO 3 – CBCAAB

13. B. Definitions Amphoteric - can be an acid or a base. Amphoteric - can be an acid or a base. NH 3 + H 2 O  NH 4 + + OH - CACBBA

14. B. Definitions F - H 2 PO 4 - H2OH2OH2OH2OHF H 3 PO 4 H 3 O + Give the conjugate base for each of the following: Give the conjugate base for each of the following: Polyprotic - an acid with more than one H + Polyprotic - an acid with more than one H +

15. B. Definitions Br - HSO 4 - CO 3 2- HBr H 2 SO 4 HCO 3 - Give the conjugate acid for each of the following: Give the conjugate acid for each of the following:

16. B. Definitions Lewis Lewis Acids are electron pair acceptors. Acids are electron pair acceptors. Bases are electron pair donors. Bases are electron pair donors. Lewis base Lewis acid

17. C. Strength Strong Acid/Base Strong Acid/Base 100% ionized in water 100% ionized in water strong electrolyte strong electrolyte - + HCl HNO 3 H 2 SO 4 HBr HI HClO 4 NaOH KOH Ca(OH) 2 Ba(OH) 2

18. C. Strength Weak Acid/Base Weak Acid/Base does not ionize completely does not ionize completely weak electrolyte weak electrolyte - + HF CH 3 COOH H 3 PO 4 H 2 CO 3 HCN NH 3

19. Neutralization An acid base reaction produces salt and water. An acid base reaction produces salt and water. An antacid soothes an overly acidic stomach by neutralizing the stomach acid. An antacid soothes an overly acidic stomach by neutralizing the stomach acid. Neutralization is the reaction of the hydronium ion and hydroxide ion to produce water. Neutralization is the reaction of the hydronium ion and hydroxide ion to produce water.

20. Salts The salt from the neutralization reaction is composed of the cation from the base and the anion from the acid. The salt from the neutralization reaction is composed of the cation from the base and the anion from the acid. Examples – Complete and balance: Examples – Complete and balance: Carbonic acid + strontium hydroxide Carbonic acid + strontium hydroxide Perchloric acid + sodium hydroxide Perchloric acid + sodium hydroxide Hydrobromic acid + barium hydroxide Hydrobromic acid + barium hydroxide Nitric acid + magnesium hydroxide Nitric acid + magnesium hydroxide

22. Acids and carbonates The products of the reaction between acids and carbonates are salt, water, and carbon dioxide. The products of the reaction between acids and carbonates are salt, water, and carbon dioxide. Acid rain can contain nitrates and sulfates and carbonates that destroy marble structures. Acid rain can contain nitrates and sulfates and carbonates that destroy marble structures. Write and balance the equations between calcium carbonate and acids from the above polyatomic ions. Write and balance the equations between calcium carbonate and acids from the above polyatomic ions.

23. Homework Page 478 # 26,28,37 Page 478 # 26,28,37