1. Chapter 25: Acids, Bases & Salts

2. I. Acids and Bases

3. A. Acids 1. produce H+ ions in solution 2. Hydronium ions (H 3 O + ) are then produced when the H + interacts with water molecules

4. B. Properties of Acids 1.Taste sour (NEVER TASTE AN ACID IN THE LAB!) 2.Corrosive- can “eat” away at metals 3.Damage tissue damage by removing water from them, causing a chemical burn.

5. Indicators 4.React with indicators- organic compound that changes color in an acid or base (organic means it is a compound that contains carbon) Examples: a. litmus paper (blue → red = acid; red → blue = base) b. universal indicator c. red cabbage juice d. phenolphthalein e. bromothymol blue

6. Litmus Paper  AciDs are ReD, and Bases are Blue  Blue to red means it is acidic  Red to blue means it is basic  No change in color means it is neutral

7. C. Common Acids 1.Citric acid (in citrus fruits) 2.Lactic acid (in milk products) 3.Acetic acid (vinegar is acetic acid + water) 4.Nitric acid 5.Sulfuric acid 6.Hydrochloric acid 7.Carbonic acid 8.Phosphoric acid

8. Writing Formulas for and Naming Acids If the anion ends in –ide, add the prefix hydro- (root of anion) and the ending –ic acid If the anion ends in ite, change to –ous acid If the anion ends in –ate, change to –ic acid

9. Name the following acids:  a. HBr b.H 3 PO 4 c.HF d.HCl e. HClO 2 f. H 2 SO 4

10. Check your work:  A. hydrobromic acid  B. phosphoric acid  C. hydrofluoric acid  D. hydrochloric acid  E. chlorous acid  F. sulfuric acid

11. Write formulas for these acids: a. sulfurous acid b.acetic acid c.nitric acid d.nitrous acid

12. Check your work: a.H 2 SO 3 b.HC 2 H 3 O 2 c.HNO 3 d.HNO 2

13. More practice  HClO 4  Oxalic acid  HBr  Hydrochloric acid  Hydrosulfuric acid

14. Acids  Examples; vinegar (acetic acid), citrus fruits (citric acid), stomach acid (hydrochloric acid), aspirin (acetylsalicylic acid); softdrinks (carbonic acid)  Four acids vital in industry: sulfuric, phosphoric, nitric, and hydrochloric acids.

15. D. Bases 1.Produce hydroxide ions (OH - ) in solution 2.Accepts H + ions from acids

16. B. Properties of Bases 1.Taste bitter (never taste to check for the presence of a base!) 2.Feel slippery (like soap, which is a base) 3.Corrosive to metals and skin 4.Can cause chemical burns 5.React with indicators 6.Red litmus paper turns blue in the presence of a base 7.Phenolphthalein turns pink

17. E. Common Bases 1.Antacids: Milk of Magnesia, “TUMS” 2.Soap 3.Ammonia (a weak base) 4.Sodium Hydroxide is used in the paper industry to separate fibers of cellulose from wood pulp. The freed cellulose fibers are made into paper. 5.Sodium Hydroxide is also in drain cleaners and oven cleaners

18. II. Strength of Acids and Bases A.Strong and Weak Acids and Bases 1. Strong Acids-- ionize almost completely in water a. Examples of Strong Acids: HCl, HNO 3, H 2 SO 4 2. Weak acids- do not completely ionize in solution a. Examples of Weak Acids: Acetic Acid

19. Strength of Acids and Bases 3. Strong Bases-- ionize almost completely in water a. Example of a Strong Base: NaOH 4. Weak bases – do not ionize completely in solution a. Examples of Weak Base: Ammonia

20. 5. Strength vs. Concentration a.Strong and Weak describe how completely acids or bases dissociate in water b.Dilute and Concentrated indicate how much acid or base is dissolved in a solution. c.It is possible to have diluted solutions of strong acids and concentrated solutions of weak acids

21. B. pH of a solution 1.measures the concentration of hydrogen ions. The greater the H + concentration, the lower the pH 2.pH can be measured using a. universal indicator b. pH meter 3. Blood pH is 7.0 – 7.8; range must be maintained for enzymes that act as catalysts for chemical reactions in the body 4. Buffers – solutions containing ions that react with additional acids or bases to minimize the effects of pH (important to keep pH in the correct range, even when acidic foods are eaten)

23. III. Salts

24. A. Neutralization 1.A chemical reaction between an acid and a base that takes place in an aqueous solution.

25. B. Salts 1.Salt- a compound formed when the negative ions from an acid combine with the positive ions from a base. 2.Acid + Base  Salt + Water 3.Salts also form as a result of single replacement reactions when acids react with metals.

26. C. Titration 1.A solution of known concentration, called the standard solution, is added slowly and carefully to a solution of unknown concentration, to which an indicator is added. 2.The Endpoint has a Color

27. D. Soaps and Detergents 1.Soaps clean so well b/c they have a polar and a nonpolar end 2.Soaps are organic salts. 3.Commercial Soaps were developed because simple soaps can react with metal ions in “hard” water, and form soap scum.

28. 4. Detergents a. have long hydrocarbon chains, like sopas, but instead of carboxylic acid groups, they have either a sulfonic acid or a phosphoric acid.

29. E. Versatile Esters 1.Esters for Flavor 2.Polyesters