Transcript Slide 1
Chapter #15 Acids and Bases 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 • • • • 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 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 Binary Acids Nomenclature • Acids always begin with H • Binary Acids that consist of 2 elements 1.Write hydro 2.Write the 2nd element 3.Change the ending to –ic 4.Write the word ACID • HF= Hydrofluoric Acid • HBr Oxyacid Nomenclature • Are acids that contain hydrogen, oxygen, and a third element. Never use Hydro 1. Write the name of the polyatomic (pg 210) 2. Change the ending to –ic or –ous (ate -ic & ite –ous) 1. Write the word ACID • H2SO4 = sulfuric acid • H3PO4 Hypo- and PerIn a series of acids • • • • HClO = HYPOchlorous Acid HClO2 = Chlorous Acid (pg 210) HClO3 = Chloric Acid (pg 210) HClO4 = PERchloric Acid Acids you SHOULD know: Strong Acids Weak Acids Sulfuric acid, H2SO4 Hydrochloric acid, HCl Nitric acid, HNO3 Phosphoric acid, H3PO4 Acetic acid, HC2H3O2 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) 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. 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 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 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 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 Examples of Bases • • • • • Sodium hydroxide (lye), NaOH Potassium hydroxide, KOH Magnesium hydroxide, Mg(OH)2 Calcium hydroxide (lime), Ca(OH)2 Alkaline basic solutions. • 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. 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 Strength of Bases • Strong bases are strong electrolytes, just as strong acids are strong electrolytes. 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). Monoprotic acids HCl HC2H3O2 HNO3 Diprotic acids Triprotic acids H2SO4 H2CO3 H3PO4 • Polyprotic give up more than one H. • 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 Base Conjugate Acid Oxides • Acidic = nonmetals • Basic= metals • Amphoteric= metalloids • MgO • Al2O3 • CO2 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. • 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. Neutralization Examples HCl + NaOH 2H3PO4 + 3Mg(OH)2 H2O + NaCl 6H2O + Mg3(PO4)2 • Information. April 27, 2007. http://www.sciencegeek.net/Chemistry/Po werpoint/Unit6/Unit6_files/frame.htm • “Cartoon”. Aug. 11, 2006. http://www.nearingzero.net/sbunch1.html