Chapter #15 Acids and Bases

1. Chapter #15Acids and Bases

2. Chapter 15.1 Some common (everyday) Acids • Sour milk= lactic acid • Vinegar= acetic acid • Tart flavor of pop= phosphoric acid • Lemons, oranges, grapefruits= citric acid • Apples= malic acid • Grape juice= tartaric acid

3. Some common Bases • Ammonia for cleaning • Lye= NaOH drain and oven cleaners • Milk of magnesia= Mg(OH)2 antacid • Al(OH)3 and NaHCO3 antacids

4. Properties of Acids • Acids taste sour • Acids effect indicators • Blue litmus turns red • Methyl orange turns red • Acids have a pH lower than 7 • Acids are proton (hydrogen ion, H+) donors • Acids react with active metals, produce H2 • Acids react with carbonates • Acids neutralize bases (acid + base = salt and water) • Acids conduct electric current

5. Binary Acids Nomenclature • Acids always begin with H • Binary Acids that consist of 2 elements • Write hydro • Write the 2nd element • Change the ending to –ic • Write the word ACID • HF= Hydrofluoric Acid • HBr

6. Oxyacid Nomenclature • Are acids that contain hydrogen, oxygen, and a third element. • Never use Hydro • Write the name of the polyatomic (pg 210) • Change the ending to –ic or –ous (ate -ic & ite –ous) • Write the word ACID • H2SO4 = sulfuric acid • H3PO4

7. Hypo- and Per- In a series of acids • HClO = HYPOchlorous Acid • HClO2 = Chlorous Acid (pg 210) • HClO3 = Chloric Acid (pg 210) • HClO4 = PERchloric Acid

8. Strong Acids Sulfuric acid, H2SO4 Hydrochloric acid, HCl Nitric acid, HNO3 Weak Acids Phosphoric acid, H3PO4 Acetic acid, HC2H3O2 Acids you SHOULD know:

9. Sulfuric Acid • Highest volume production of any chemical in the U.S. • Used in the production of paper • Used in production of fertilizers • Used in petroleum refining • Used in Automobile batteries • Thick clouds of sulfuric acid are a feature of the atmosphere of Venus. (image provided by NASA)

10. Nitric Acid • Used in the production of fertilizers • Used in the production of explosives • Nitric acid is a volatile acid – its reactive components evaporate easily • Stains proteins (including skin!) • Used in making rubber, plastics, dyes, and pharmaceuticals.

11. Phosphoric Acid • A flavoring agent in sodas • Used in the manufacture of detergents • Used in the manufacture of ceramics • Used in the manufacture of fertilizers • Not a common laboratory reagent

12. Hydrochloric Acid • Used in the pickling of iron & steel • Used as a cleaning agent, in food processing & in activation of oil wells. • Used to purify magnesium from sea water • Part of gastric juice, it aids in the digestion of protein • Sold commercially as “Muriatic acid” Swimming pools • Stomach ACID

13. Acetic Acid • Used in the manufacture of plastics • Used in making food supplements Lysine – amino acid (Jurassic Park) • Used as a fungicide • Acetic acid is the acid present in vinegar

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

15. Examples of Bases • Sodium hydroxide (lye), NaOH • Potassium hydroxide, KOH • Magnesium hydroxide, Mg(OH)2 • Calcium hydroxide (lime), Ca(OH)2 • Alkaline basic solutions.

16. Arrhenius acid is a chemical that increases the concentration of hydrogen ions, H+, in aqueous solution. • Arrehenius base is a chemical that increases the concentration of hydroxide ions, OH-, in aqueous solution.

17. Strong Acids vs. Weak Acids • Strong acids are assumed to be 100% ionized in solution (good proton donors). HCl H2SO4 HNO3 • Weak acids are usually less than 5% ionized in solution (poor proton donors). H3PO4 HC2H3O2 Organic acids

18. Strength of Bases • Strong bases are strong electrolytes, just as strong acids are strong electrolytes.

19. Chapter 15.2 • Bronsted-Lowry Acid is a Proton Donors (H+) • Bronsted-Lowry Base is a proton acceptor • Bronsted-Lowry acid-base reaction protons are transferred from one reactant (Acid) to another (base).

20. Monoprotic acids Diprotic acids Triprotic acids HCl H2SO4H3PO4 HC2H3O2H2CO3 HNO3 • Polyprotic give up more than one H.

21. Conjugate base is the species that remains after a Bronsted-Lowry acid has given up (loses) a proton. • Conjugate acid is the species from when a Bronsted-Lowry bases gains a proton. HF + H2O F- + H3O+ Acid Base Conjugate BaseConjugate Acid

22. Oxides • Acidic = nonmetals • Basic= metals • Amphoteric= metalloids • MgO • Al2O3 • CO2

23. Chapter 15.3 • Neutralization is the reaction of hydronium ions and hydroxide ions to form water molecules. • Salt is an ionic compound composed of a cation from a base and an anion from an acid.

24. Lewis acid is an atom, ion, or molecule that accepts an electron pair to form a covalent bond. • Lewis base is an atom, ion, or molecule that donates an electron pair to form a covalent bond. • A Lewis acid-base reaction is the formation of one or more covalent bonds between an electron-pair donor and an electron-pair acceptor.

25. Neutralization Examples HCl + NaOH H2O + NaCl 2H3PO4 + 3Mg(OH)2 6H2O + Mg3(PO4)2

26. Information. April 27, 2007. http://www.sciencegeek.net/Chemistry/Powerpoint/Unit6/Unit6_files/frame.htm • “Cartoon”. Aug. 11, 2006. http://www.nearingzero.net/sbunch1.html