1. Acids and Bases

2. What are acids and bases?
Acid – A substance that produces hydronium ions (H3O+) in water.
This is done by the substance losing a hydrogen ion (H+) to a water molecule.
Strong Acid – an acid that ionizes completely (nearly 100%) in water.
Example: HCl + H2O → H3O+ + Cl-
Excellent conductors of electricity in solution.
Weak Acid – only a small fraction (generally less than 5%) of the molecules ionize in water.
Example: HClO + H2O → H3O+ + ClO-
Conduct electricity somewhat (weak electrolytes)

3. Carboxylic Acids (organic acids) – Contain
Generally weak acids – lose the H that is bonded to the O.
Properties of Acids:
Low pH (below 7)
Sour taste (example: citric acid)

4. Bases – Create hydroxide ions (OH-) in aqueous solution
Bases – Create hydroxide ions (OH-) in aqueous solution. They either contain OH- or remove H+ from water.
Example:
Strong Base – Ionizes completely in solution (example: NaOH)
Weak Base – small fraction of molecules create OH- in water (Example: NH3) NH3 + H2O → NH4+ + OH-
Properties of Bases:
High pH (above 7)
Taste Bitter
Feel Slippery

5. Neutralization Reaction
A reaction in which an acid and a base react to form water.
H3O+ + OH- → 2 H2O
2NaOH + H2SO4 → Na2SO4 + 2H2O
KOH + HCl →

6. pH

7. pH and pOH pH = -log [H3O+] pOH = - log [OH-] pH + pOH = 14.00
pH of 7 is neutral
pH greater than 7 is basic (pOH less than 7)
pH less than 7 is acidic (pOH greater than 7)
The greater the concentration of hydronium ions, the lower the pH and higher pOH, and vice versa.