1. Chapters 15 and 16

2. Properties of Acids and Bases Acids H pH less than 7 Sour taste Corrosive Conduct electric current Ionization Bases OH pH greater than 7 Bitter taste/slippery Corrosive Conduct electric current Dissociation

3. COMMON ACIDS Acetic acid - vinegar Sulfuric acid – car batteries Nitric acid - fertilizer/explosive Hydrochloric acid - Stomach - pool cleaner (muriatic acid) COMMON BASES Ammonia – NH 3 KOH – soap NaOH – drain opener

4. STRENGTH VS. How completely it ionizes or dissociates. (will not change) CONCENTRATION Measurement of how much acid or base is in a solution. (can be changed)

5. Acids **Balance charges **Do not name “Hydrogen” Hydro _____________ic __________________ic __________________ous “ide” “ate” “ite”

6. Indicators – React with substances to produce color changes. Acid Base Litmus paperred blue Phenolphthaleinclear pink Bromothymol blueyellow blue Universal indicatorred-yellow blue-purple

7. Arrhenius acid – Increases concentration of Hydrogen (H + ) or Hydronium ions (H 3 O + ). Arrhenius base – Increases concentration of Hydroxide ions (OH - ).

8. Bronsted-Lowry acid – Proton donor Bronsted-Lowry base – Proton acceptor HCl + NH 3 → NH 4 + + Cl -

9. pH Scale pH = potential of hydrogen Ranges from 0 – 14 The lower the pH, the more acidic (more hydrogen). The higher the pH, the stronger the base (less H). pH of 7 is neutral.

10. pH = - log [H 3 O + ] pOH = - log [OH - ] pH + pOH = 14 [H 3 O + ] = (2 nd ) (log) (-pH) [OH - ] = (2 nd ) (log) (-pOH)

11. Neutralization Reactions A reaction between an acid and a base Produces water and a salt.