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Honors Chemistry Acids and Bases

Honors Chemistry Acids and Bases. 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. Review of Acid Names. Binary Acids (with “hydro” in name) “-ide”  “-ic acid” w/ “hydro” prefix

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Honors Chemistry Acids and Bases

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  1. Honors ChemistryAcids and Bases

  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 • Binary Acids (with “hydro” in name) • “-ide”  “-ic acid” w/ “hydro” prefix • HCl – hydrochloric acid • HBr – hydrobromic acid • H2S – hydrosulfuric acid • Hydrophosphoric acid – H3P • Hydroiodic acid - HI

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

  5. Review of Acid Names • Oxyacids (made w/ polyatomic ions) • “-ate”  “-ic acid” • “-ite”  “-ous acid” • HClO3 – chloric acid (from chlorate) • H2SO4 – sulfuric acid (from sulfate) • H2SO3 – sulfurous acid (from sulfite) • Perchloric acid – HClO4 • Phosphoric acid – H3PO4 • Phosphorous acid – H3PO3

  6. Acid Reactions • Three ways to neutralize an acid… • Acid + Metal • Acid + Base • Acid + Carbonate • Type 1: Acid + Metal  Salt + H2 • HA + M  MA + H2 • Example: Hydrochloric acid + potassium (Explosive!) • 2 HCl + 2 K  2 KCl + H2

  7. Acid Reactions • Type 2: Acid + Base  Salt and Water • 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

  8. Acid Reactions • Type 3: Acid + Carbonate  Salt + CO2 + H2O • HA + MCO3  MA + CO2 + H2O • A C S • Example: sulfuric acid and barium carbonate • H2SO4 + BaCO3 BaSO4 + CO2 + H2O • A C S

  9. Review • Predict the products of the following reactions (do not balance): • HCl + Na  • H2SO4 + KOH  • HBr + K2CO3  • Extra challenge: use all three reaction types to produce KCl as the product salt.

  10. Review • Predict the products of the following reactions (do not balance): • HCl + Na  NaCl + H2 • H2SO4 + KOH  K2SO4 + H2O • HBr + K2CO3  KBr + CO2 + H2O • Extra challenge: use all three reaction types to produce KCl as the product salt.

  11. 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 (titration lab) Orange in methyl orange (another indicator) 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

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

  13. 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. Electrolytes improve the flow of electricity in a solution, which your nerves need to transmit electrical signals throughout your body. http://www.youtube.com/watch?v=uxieMOdo6IU Properties of Acids and Bases

  14. 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

  15. BrØnsted-Lowry Acid/Base – 1923 J. N. BrØnsted and T.M. Lowry A BrØnsted-Lowry acid is a proton (H+) donor HCl, H2SO4, H2O (in some cases) An BrØnsted-Lowry base is a proton acceptor NH3 (can become NH4+), H2O can become H3O+ Acid Definitions

  16. HCl + NH3  NH4+ + Cl- This is an example of a Bronsted-Lowry acid/base reaction. The proton on the acid (HCl) is accepted by the base (NH3) After the HCl loses the proton, Cl- is now considered a base (because it could possibly receive a proton again) – called a conjugate base Same with the NH3 accepting the proton – the NH4+ could give the proton away, making NH4+ a conjugate acid. HCl + NH3  NH4+ + Cl- Acid Base C.A. C.B. Acid/Base Reactions

  17. Water, because it is pH neutral, can act as both an acid and a base. Amphoteric – both an acid and a base H2O + H2O  H3O+ + OH- Acid Base C.A. C.B. This happens all the time – the reason water is neutral is because at all times, there are equal amounts of H3O+ and OH- !! Water

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