Acids and Bases

Definitions Acids – produce H+ Bases - produce OH- Acids – donate H+ Bases – accept H+ Arrehenius Bronsted-Lowry

Examples HCl Lemon Juice Soda NaOH Bleach Soap H2SO4 Acid Rain Vinegar Acids HCl Lemon Juice Soda NaOH Bleach Soap H2SO4 Acid Rain Vinegar KOH Ammonia M.O.M Bases

Properties of Acids pH < 7.0 Taste Sour React with metals Turn litmus paper red

Properties of Bases pH > 7.0 Taste Bitter Slippery, soapy feeling Turn litmus paper blue

Acids & Bases Conduct electricity (electrolytes) React with indicators

Indicators Universal Indicator Chemicals which change colors when they are put into acids or bases.

Acid + Base  Water + Ionic Compound Acid/Base Reactions (Neutralization Reactions) Acid + Base  Water + Ionic Compound HCl + KOH  HOH + KCl H2SO4 + 2KOH  2H2O + K2SO4

What is pH? measures the concentration of H+ ions (How acidic or basic a solution is) pH = -log[H+] If [H+] = 1 x 10-4, then pH = 4 If [H+] = 1 x 10-13, then pH = 13 If [H+] = 1 x 10-7, then pH = 7

pH Scale Acid Neutral Base H+ OH- 1 2 3 4 5 6 7 8 9 10 11 12 13 14 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Urine Blood Saliva Bleach Ammonia Sea Water Pure Water Baking Soda Gastric Juice Tomato Juice Black Coffee Milk of Magnesia Battery Acid, HCl Orange Juice, Soda Lemon Juice, Vinegar Liquid Draino, NaOH

pH and pOH [H+][OH-] = 10-14 pH + pOH = 14 If [OH-] = 10-8 M, what is the pH? the pOH = 8, so the pH must be 14 – 8 So the pH = 6