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Acids and Bases Strong Acids, strong bases and pH Bronsted-Lowry Model of Acids and Bases Acid is a proton donor, base is a proton acceptor. HB(aq) + A-(aq) ↔ HA(aq) + B-(aq) HA and HB are acids, A- and B- are bases HB & B- and HA & A- are conjugate acidbase pairs. Watch this animation http://www.mhhe.com/physsci/chemistry /essentialchemistry/flash/acid13.swf Watch this animation about acids and bases in solution http://preparatorychemistry.com/Bishop_ Neut_frames.htm Watch the “acid animation” at the same site – look at the menu on the left Demo - A Voice Activated Reaction Acidic and Basic Water Solutions In any aqueous solution, there is an equilibrium between H3O+ (H+) ions and OHions. 2 H2O ↔ H3O+(aq) + OH-(aq) Kw = [H3O+][OH-] = 1.0 x 10-14 @25oC So in pure water: [H+] = [OH-] = 1.0 x 10-7 M A neutral solution Acidic solutions: [H+] > 1.0 x 10-7 M > [OH-] Basic solutions: [OH-] > 1.0 x 10-7 M > [H+] Ex In sea water, [H+] = 5 x 10-9 M [OH-] = ? pH Scale pH = -log[H+] neutral solution: pH = 7.0 acidic solution: pH < 7.0 basic solution: pH > 7.0 Look at the animation at: http://www.johnkyrk.com/pH.html ex Suppose [H+] = 2.4 x 10-6 M; calculate pH Ex Suppose pH = 8.68; Calculate [H3O+] pOH = -log[OH-] [H+][OH-] = 1 x 10-14 pH + pOH = 14 Watch the music video http://www.youtube.com/watc h?v=u9nOIZDdvRw Here is the notes quiz https://docs.google.com/spreadsheet/embeddedform?formkey=dGhuNE53RkdkV1 ZJc1BGdGFQeEEzVWc6MQ
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