1. Acid/base stoichiometry, nomenclature, definitions, reaction equations,

2.  Lewis  Acid: A compound that can receive an electron pair  Base: A compound that can donate an electron pair  Bronsted-Lowry  Acid: A substance that has the ability to DONATE a proton to another substance  Base: A substance that has the ability to ACCEPT a proton from another substance HCl+H 2 0  H 3 0 + + Cl -  Arrhenius  Acid: Substance that when dissolved in water increases the H + ion concentration  Base: Substance that when dissolved in water increases the OH - ion concentration

3.  pH=log[H + ]  [H + ]=10 -pH  K w =1x10 -14

4.  Strong acids and bases dissociate completely

5. IndicatorAppearance in AcidAppearance in Base Methyl OrangeRedYellow Bromphenol BlueYellowBlue PhenolpthaleinColorlessRed  An indicator is a weak acid or base that changes color in the presence of an acid or base

6.  Example set-ups of typical stoichiometry uses for acids/bases

7.  The net reaction equation between a strong acid and a strong base is H + + OH -  H 2 O The substances that were aqueous and do not react are spectator ions, and therefore not in the net reaction.

8.  Acids often begin with an “H”, bases often end in an “OH”  Exception:CH 3 COOH (acetic acid)  Acid naming:  Example: HF Hydrogen fluoride as an acid is called hydrofluoric acid AnionAcid -ideHydro____ic -ate-ic -ite-ous

9.  http://www.sciencegeek.net/Chemistry/eTe xt/U6/6h.html http://www.sciencegeek.net/Chemistry/eTe xt/U6/6h.html  Chemistry the Central Science 11e  http://library.thinkquest.org/C006669/data/ Chem/reactions/acidbase.html http://library.thinkquest.org/C006669/data/ Chem/reactions/acidbase.html