CHAPTER%2019.1%20ACID-BASE%20THEORIES - PowerPoint PPT Presentation

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ARRHENIUS ACIDS. Acids are hydrogen-containing compounds that ionize (dissolve) to yield hydrogen ions H+ in aqueous solutions – PowerPoint PPT presentation

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Title: CHAPTER%2019.1%20ACID-BASE%20THEORIES


1
CHAPTER 19.1 ACID-BASE THEORIES
2
OBJECTIVE
  • Compare and contrast acids and bases as defined
    by the theories of Arrhenius and Brønsted-Lowry

3
ACIDS AND BASES
  • Foods
  • Acids have a tart or sour taste
  • Bases have a bitter taste
  • Bases feel slippery
  • Aqueous solutions of acids and bases are
    electrolytes
  • Some are strong, some are weak
  • Acids bases will change color when an acid-base
    indicator is added
  • Acids bases react to form water and salt

4
ARRHENIUS ACIDS
  • Acids are hydrogen-containing compounds that
    ionize (dissolve) to yield hydrogen ions H in
    aqueous solutions

5
ARRHENIUS ACIDS
  • Monoprotic acid acids containing 1 ionizable
    hydrogen
  • Example nitric acid, HNO3
  • Diprotic acid acids containing 2 ionizable
    hydrogen
  • Example sulfuric acid, H2SO4
  • Tripotic acid acids containg 3 ionizable
    hydrogen
  • Example phosphoric acid, H3PO4

6
ARRHENIUS ACIDS
  • Not all acids with hydrogen will release hydrogen
    ions
  • Only those with strong polar bonds are ionizable
    hydrogen joined by a very electronegative element
  • Hydrogen has an electronegativity of 2.1
  • Electronegativity increases up a column and to
    the right
  • Common Acids
  • HCl, HNO3, H2SO4, H3PO4, CH3COOH, H2CO3

7
ARRHENIUS BASES
  • Compounds that ionize to yield hydroxide ions OH-
    in aqueous solutions

8
ARRHENIUS BASES
  • Group IA elements, alkali metals, react with
    water to produce basic solutions
  • NaOH(s) H2O(l) ? Na(aq) OH-(aq)
  • Group IIA element, alkaline earth metals, react
    with water but arent very soluble
  • Common bases
  • KOH, NaOH, Ca(OH)2, Mg(OH)2

9
BRØNSTED-LOWRY ACIDS BASES
  • Arrhenius definition of acids and bases fails to
    consider compounds that have acidic and basic
    properties that dont have a related hydroxide
  • Sodium Bicarbonate (Na2CO3) is a base
  • Ammonia (NH3) is a base

10
BRØNSTED-LOWRY ACIDS BASES
  • Brønsted-Lowry theory defines an acid as a
    hydrogen-ion donor, and a base as a hydrogen-ion
    acceptor
  • All acids and bases as defined by the Arrhenius
    theory are acids and bases according to the
    Brønsted-Lowry theory

11
BRØNSTED-LOWRY ACIDS BASES
  • Ammonia, NH3
  • NH3(aq) H2O(l) ? NH4(aq) OH-(aq)
  • Hydrogen-ion donor water
  • Brønsted-Lowry Acid
  • Hydrogen-ion acceptor NH3
  • Brønsted-Lowry Base

12
BRØNSTED-LOWRY ACIDS BASES
  • Conjugate Acids Bases
  • Conjugate acid particle formed when a base
    gains a hydrogen ion
  • Conjugate base particle formed when an acid has
    donated a hydrogen ion
  • Conjugate acid-base pair two substances related
    by the loss or gain of a single hydrogen ion

NH3(aq) H2O(l) ? NH4(aq) OH-(aq)
13
BRØNSTED-LOWRY ACIDS BASES
  • Hydrochloric Acid, HCl
  • HCl(g) H2O(l) ? H3O(aq) Cl-(aq)
  • Hydrogen-ion donor HCl
  • Brønsted-Lowry Acid
  • Hydrogen-ion acceptor water
  • Brønsted-Lowry Base

14
BRØNSTED-LOWRY ACIDS BASES
  • Amphoteric A substance that can act as an acid
    or a base
  • Example water
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