logging in or signing up Acids and Bases gerilyn Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: (To copy code, click on the text box) Embed: URL: Thumbnail: WordPress Embed Customize Embed The presentation is successfully added In Your Favorites. Views: 129 Category: Entertainment License: All Rights Reserved Like it (0) Dislike it (0) Added: June 05, 2010 This Presentation is Public Favorites: 0 Presentation Description No description available. Comments Posting comment... Premium member Presentation Transcript Acids and Bases : Acids and Bases Bronsted-Lowry Definition : Bronsted-Lowry Definition ACIDS are proton donors; BASES are proton acceptors. HCl + H2O H3O+ + Cl- acid base conjugate conjugate acid base H2O + H2O H3O+ + OH- WATER is amphoteric with properties of ACIDS & BASES Properties of Acids : Properties of Acids Sour taste Electrolytes React with metals to produce hydrogen gas and a salt Produce hydronium ion, H3O+, due to ionization in water (Arrhenius definition) pH <7 Strong Acids : Strong Acids Strong acids (100% ionization) HCl hydrochloric acid HBr hydrobromic acid HI hydroiodic acid HNO3 nitric acid H2SO4 sulfuric acid HClO4 perchloric acid HIO4 periodic acid Weak Acids : Weak Acids Weak acids (small % ionization) CH3COOH acetic acid HCN hydrocyanic acid HF hydrofluoric acid HNO2 nitrous acid H2SO3 sulfurous acid HOCl hypochlorous acid H3PO4 phosphoric acid Properties of Bases : Properties of Bases Slippery to the touch React with acids to form water and a salt (neutralization) Produce hydroxide ion, OH-, in aqueous solution pH >7 Strong and Weak Bases : Strong and Weak Bases Strong Bases Weak Bases NaOH sodium hydroxide KOH potassium hydroxide Ca(OH)2 calcium hydroxide Ba(OH)2 barium hydroxide Na3PO4 sodium phosphate NH3 ammonia Na2CO3 sodium carbonate K2CO3 potassium carbonate Writing dissociation equations for acids and bases. : Writing dissociation equations for acids and bases. HCl H+ (aq) + OH-(aq) H2SO4 2H+ (aq) + SO4-(aq) NaOH Na+(aq) + OH-(aq) Ca(OH)2 Ca+(aq) + 2OH-(aq) Calculating pH and pOH from concentration : Calculating pH and pOH from concentration pH= -log[H+] To solve for pH: plug the H+ into the equation above [H+]= 10^(-)(pH) When given the pH level, plug the pH into the equation above Don’t forget about sig figs! Calculating the concentration of hydrogen ion in an aqueous solution given the hydroxide ion concentration and Kw : Calculating the concentration of hydrogen ion in an aqueous solution given the hydroxide ion concentration and Kw -14 Kw = 1.0 x 10 Kw = [OH-][H3O+] [OH-] = .0001 M -14 -10 [H3O+] = 1.0 x 10 = 1.0 x 10 M .0001 You do not have the permission to view this presentation. In order to view it, please contact the author of the presentation.
Acids and Bases gerilyn Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: (To copy code, click on the text box) Embed: URL: Thumbnail: WordPress Embed Customize Embed The presentation is successfully added In Your Favorites. Views: 129 Category: Entertainment License: All Rights Reserved Like it (0) Dislike it (0) Added: June 05, 2010 This Presentation is Public Favorites: 0 Presentation Description No description available. Comments Posting comment... Premium member Presentation Transcript Acids and Bases : Acids and Bases Bronsted-Lowry Definition : Bronsted-Lowry Definition ACIDS are proton donors; BASES are proton acceptors. HCl + H2O H3O+ + Cl- acid base conjugate conjugate acid base H2O + H2O H3O+ + OH- WATER is amphoteric with properties of ACIDS & BASES Properties of Acids : Properties of Acids Sour taste Electrolytes React with metals to produce hydrogen gas and a salt Produce hydronium ion, H3O+, due to ionization in water (Arrhenius definition) pH <7 Strong Acids : Strong Acids Strong acids (100% ionization) HCl hydrochloric acid HBr hydrobromic acid HI hydroiodic acid HNO3 nitric acid H2SO4 sulfuric acid HClO4 perchloric acid HIO4 periodic acid Weak Acids : Weak Acids Weak acids (small % ionization) CH3COOH acetic acid HCN hydrocyanic acid HF hydrofluoric acid HNO2 nitrous acid H2SO3 sulfurous acid HOCl hypochlorous acid H3PO4 phosphoric acid Properties of Bases : Properties of Bases Slippery to the touch React with acids to form water and a salt (neutralization) Produce hydroxide ion, OH-, in aqueous solution pH >7 Strong and Weak Bases : Strong and Weak Bases Strong Bases Weak Bases NaOH sodium hydroxide KOH potassium hydroxide Ca(OH)2 calcium hydroxide Ba(OH)2 barium hydroxide Na3PO4 sodium phosphate NH3 ammonia Na2CO3 sodium carbonate K2CO3 potassium carbonate Writing dissociation equations for acids and bases. : Writing dissociation equations for acids and bases. HCl H+ (aq) + OH-(aq) H2SO4 2H+ (aq) + SO4-(aq) NaOH Na+(aq) + OH-(aq) Ca(OH)2 Ca+(aq) + 2OH-(aq) Calculating pH and pOH from concentration : Calculating pH and pOH from concentration pH= -log[H+] To solve for pH: plug the H+ into the equation above [H+]= 10^(-)(pH) When given the pH level, plug the pH into the equation above Don’t forget about sig figs! Calculating the concentration of hydrogen ion in an aqueous solution given the hydroxide ion concentration and Kw : Calculating the concentration of hydrogen ion in an aqueous solution given the hydroxide ion concentration and Kw -14 Kw = 1.0 x 10 Kw = [OH-][H3O+] [OH-] = .0001 M -14 -10 [H3O+] = 1.0 x 10 = 1.0 x 10 M .0001