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.

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

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

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

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)

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)

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

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

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

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

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

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

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