1. Acids and Bases SNC2D

2. Some Properties of Acids  Sour taste  Water soluble  Very reactive  Conduct electricity  Can act as a catalyst  Corrosive  Increase the hydrogen ion (H 1+ ) concentration of a solution  Low pH (see chapter 7.3 The pH Scale)

3. Binary Acids  HX (where X is typically a halogen)  HX is typically a gas (HX (g) )  e.g. hydrogen chloride (HCl (g) )  When dissolved in water they form an acid  e.g. hydrochloric acid (HCl (aq) )

4. Oxyacids and Organic Acids  Oxyacids are acids where hydrogen is attached to a polyatomic ion that contains oxygen  e.g. phosphate (PO 4 3- ) would give us phosphoric acid (H 3 PO 4 )  Organic acids are those found in nature and contain carbon  e.g. vinegar (acetic acid) and ascorbic acid (vitamin C)

5. Some Properties of Bases  Bitter taste  Water soluble  Very reactive  Conduct electricity  Caustic  Are also described as alkaline  Increase the hydroxide ion (OH 1- ) concentration of a solution  High pH (see chapter 7.3 The pH Scale)

6. Typical Bases  Bases usually contain the hydroxide ion (OH 1- )  e.g. sodium hydroxide (NaOH)  Some are more difficult to recognize  bicarbonate (HCO 3 1- ) looks like an acid but can act as a base by taking a hydrogen ion from water and leaving behind the hydroxide ion  HCO 3 1- + H 2 O  H 2 CO 3 + OH 1-

7. Indicators  Indicators are compounds that change colour to identify an acid or base.  Litmus  red = acid blue = base  Wide range pH  Phenolphthalein  Bromthymol Blue

8. Neutralization Reactions  acid + base  salt + water  HCl + NaOH  NaCl + H 2 O  HNO 3 + KOH  KNO 3 + H 2 O

9. Credits  http://commons.wikimedia.org/wiki/File:Hydrochloric_acid_ammonia.jpg http://commons.wikimedia.org/wiki/File:Hydrochloric_acid_ammonia.jpg