1. CH 14 Acids and Bases 14.1 Properties of Acids and Bases
Sour taste, change the color of acid-base indicators, some react with metals to release hydrogen gas (H2), react with bases to produce salt and water, and conduct electric current.

2. Binary acid: Nomenclature Oxyacid 2 elements: H and an electronegative
Begins with hydro-
Root of name of second element follows prefix
Ends with -ic
Oxyacid
H, O, and third nonmetal

3. Main acids in industry
Sulfuric Acid: petroleum refining, fertilizers, production metals/paper/paint/dyes/batteries, removes water well
Nitric Acid: volatile/unstable so must be dissolved in water, used in explosives, production rubber/ plastic/ dyes/ pharmaceuticals
Phosphoric Acid: fertilizers and animal feed, diluted it’s used for flavoring beverages or cleaning machinery
Hydrochloric Acid: in stomach for digestion, pickling metals to remove impurities, cleaning and food processing industries
Acetic Acid: vinegar contains acetic acid, used synthesize chemicals, production of food supplements

4. Properties of bases
Taste bitter, change color of acid-base indicators, feels slippery, react with acids to produce salts and water, and conduct an electric current
Arrhenious acids: increases H+ ions and Arrhenious bases: increases OH- ions
Strength of acids:
Strong acids: ionize completely in aq solution
Weak acids: release few H+ ions in aq solution

5. Aqueous solutions of bases
Metal cation with OH- anions
Ionic compounds
Strength of bases
Depends on extent OH- ions dissociate in soln (just like acids)

6. 14.2 Acid-Base Theories Bronsted-Lowry Acid Bronsted-Lowry Base
Molecule/ion that is proton donor
Bronsted-Lowry Base
Molecule/ion that is proton acceptor
Acid-base reaction
-prtotons are transferred from one reactant (acid) to the other (base)

7. Monoprotic Acid: acid that can only donate 1 proton (H+) per molecule
Polyprotic Acid: acid that can donate more than one proton (H+) per molecule
Diprotic Acid: donate 2 protons
Triprotic Acid: donate 3 protons

8. Lewis Acid: atom/ion/molecule accepts e- pair to form a covalent bond
Lewis Base: atom/ion/molecule that donates an e- pair to form a covalent bond
Lewis acid-base reaction: formation of one or more covalent bonds between e- pair donor and e- pair acceptor
Pd 2 stopped Friday

9. 14.3 Acid-Base Reactions Bronsted-Lowry conjugate acid-base pairs
Conjugate base: what remains after Bronsted-Lowry acid has given up proton
Conjugate acid: what is formed when Bronsted- Lowry base gains a proton
Strength of conjugative acids-bases: depends on strength of acids and bases involved

10. Use strengths of acids and bases to predict outcomes of reactions (pg 459)

11. Amphoteric: act as either an acid or a base
Water
OH- Hydroxyl group

12. Neutralization Produces water and salt
Hydronium ions and hydroxide ions form water
Salt is ionic compound composed of cation from base and anion from acid

13. Acid precipitation Caused by industrial processes
Compounds dissolve in water
Acid rain damages buildings, plants, habitats, etc.