1. Distinguishing Acids and Bases
donates H+
donates OH- accepts H+
Jennifer Simmons

2. Properties of Acids and Bases
pH less than 7 corrosive, can feel irritating taste sour usually have H+ in formula react with metals neutralize bases
pH higher than 7 feel slippery taste bitter often have OH- in formula dissolve oils and fats neutralize acids

3. Acids Donate Protons HNO3  H+ + NO3-
H+ is donated by nitric acid, HNO3
H+ = proton
The concentration of H+ determines pH
Lower pH = higher concentrations of H+

4. Bases Accept Protons Na2CO3 + H+  HCO3- + 2 Na+
H+ is accepted by Na2CO3, a base
The concentration of H+ determines pH
Bases remove H+ from the solution, which raises the pH.

5. Formulas of Acids
Since acids are H+ donors, their formulas can often be recognized by a leading H: HNO3 nitric acid H2CO3 carbonic acid HCl hydrochloric acid H2SO4 sulfuric acid HClO3 chloric acid

6. Formulas of Bases
Bases that contain OH- can be recognized by their formula:
NaOH sodium hydroxide
KOH potassium hydroxide
Mg(OH) magnesium hydroxide
Ca(OH) calcium hydroxide
Ba(OH) barium hydroxide

7. Reactions with Indicators
Acids and bases react differently with chemicals known as indicators.
We can use indicators to identify whether a substance is an acid or a base.
There are 2 common indicators:
Litmus
Phenolphthalein

8. Litmus Indicator Litmus can be used to identify acids and bases:
Blue litmus paper turns red in acids (stays blue in bases)
Red litmus paper turns blue in bases (stays red in acids)

9. Phenolphthalein Indicator
Phenolphthalein in a neutral solution is pale pink. Phenolphthalein turns colorless in an acid. Phenolphthalein turns dark pink in a base.