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Chemistry Acids and Bases Properties of Acids and Bases

Chemistry Acids and Bases Properties of Acids and Bases. Periodic Tables Required ION CHARTS REQUIRED Calculators Optional. Review of Acid Names. Binary Acids (with “hydro” in name) “-ide”  “-ic acid” w/ “hydro” prefix HCl HBr H 2 S Hydrophosphoric acid Hydroiodic acid.

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Chemistry Acids and Bases Properties of Acids and Bases

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  1. ChemistryAcids and BasesProperties of Acids and Bases Periodic Tables Required ION CHARTS REQUIRED Calculators Optional

  2. Review of Acid Names • Binary Acids (with “hydro” in name) • “-ide”  “-ic acid” w/ “hydro” prefix • HCl • HBr • H2S • Hydrophosphoric acid • Hydroiodic acid

  3. Review of Acid Names • Oxyacids (made w/ polyatomic ions) • “-ate”  “-ic acid” • “-ite”  “-ous acid” • HClO3 • H2SO4 • H2SO3 • Perchloric acid • Phosphoric acid • Phosphorous acid

  4. Arrhenius Acid/Base – 1900 Svante Arrhenius An Arrhenius acid is a compound that increases the amount of H+ in solution. HCl, H2SO4 An Arrhenius base is a compound that increases the amount of OH- in solution. Ba(OH)2, NaOH Acid Definitions

  5. BrØnsted-Lowry Acid/Base – 1923 J. N. BrØnsted and T.M. Lowry A BrØnsted-Lowry acid is a proton (H+) donor HCl + H2O  Cl- + H3O+ donor acceptor An BrØnsted-Lowry base is a proton acceptor NH3+ H2O  NH4+ + OH- acceptor donor Acid Definitions

  6. Water, because it is pH neutral, can act as both an acid and a base. Amphoteric – both an acid and a base Can release H+ to become OH- Can accept H+ to become H3O+ (hydronium) This happens all the time – the reason water is neutral is because at all times, there are equal amounts of H3O+ and OH- !! Water

  7. Acids, bases, and soluble salts dissociate, or separate into ions when dissolved in water. HCl(g) H+(aq) + Cl-(aq) Increase in H+ = Acid NaOH(s)  Na+(aq) + OH-(aq) Increase in OH- = Base NaCl(s) Na+(aq) + Cl-(aq) Doesn’t affect H+ or OH- = Neutral (salt) Dissociation

  8. Acid Dissociation Arrhenius: HBr Bronsted-Lowry: HBr + H2O  Base Dissociation Arrhenius: Ca(OH)2  Bronsted-Lowry: NH3 + H2O  Practice

  9. Over the years, there have been changes to the way an acid or base was defined. Nevertheless, they exhibit the same properties regardless of definition. Properties of Acids Colorless in phenolpthalein React with most metals Taste sour (citric acid in lemon juice) Turns litmus paper red (Red = Acid) pH 0-6.99 Properties of Acids and Bases

  10. Properties of Bases Bitter tasting (milk is a weak base) Pink in phenolpthalein Do not react with metals Turns litmus paper blue (Blue = Base) pH 7.01-14 Feel slippery (like soap!) Properties of Acids and Bases

  11. Properties of Both They both sting wounds & flesh They are both electrolytes Both produce salts in reactions An electrolyte is an ion in solution. NaCl  Na+(aq) + Cl-(aq) Any salt dissolved in water is an electrolyte. http://www.youtube.com/watch?v=uxieMOdo6IU Properties of Acids and Bases

  12. Acid Reactions • Two main ways to neutralize an acid… • Acid + Metal • Acid + Base • Type 1: Acid + Metal  Salt + H2 • HA + M  MA + H2 • Format: Single Replacement • Example: Hydrochloric acid + potassium (Explosive!) • 2 HCl + 2 K  2 KCl + H2

  13. Acid Reactions • Type 2: Acid + Base  Salt and Water • Format: Double Replacement • HA + BOH  AB + H2O • A B S W • Example: Hydrobromic acid and barium hydroxide • 2 HBr + Ba(OH)2 BaBr2 + 2 H2O • A B S W

  14. Review • Predict the products of the following reactions - • HCl + Na  • H2SO4 + KOH 

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