1. Strengths of Acids and Bases

2. Electrical Conductivity
Acidic and basic solutions conduct electricity.
We can see a current being conducting by electrocuting a pickle. A pickle has been soaked with a solution of vinegar and salt. (ions are from the acid and Na+ and Cl-) The ions are able to carry the current.
What color do you think the light emitted will be? Why would it be that color?
You tube-electrocuting a pickle

3. Strong acids produce a strong electric current = strong electrolyte
Strengths of Acids
Acids that completely ionize (dissociate) are called strong acids.
Strong acids produce a strong electric current = strong electrolyte
HCl(aq) +H2O(l)  H3O+(aq) + Cl-(aq)
(notice there is a one way arrow meaning it completely ionizes and does not reform HCl)

4. Strengths of Acids
Weak acids partially ionize in solutions = weak electrolyte
Produce fewer ions and cannot conduct electricity as efficiently as strong acids
HC2H3O2(aq) +H2O(l)  H3O+(aq) + C2H3O2-(aq)
(notice there is a two way arrow meaning it partially ionizes and does reform HC2H3O2)

5. Six Strong Acids Hydrochloric acid: HCl Hydrobromic acid: HBr
Hydroiodic acid: HI 
Sulfuric acid: H2SO4 
Nitric acid: HNO3
Perchloric acid: HClO4
These acids completely dissociate in water.

6. Eight Strong Bases Lithium hydroxide: LiOH Sodium hydroxide: NaOH
Potassium hydroxide: KOH 
Rubidium hydroxide: RbOH 
Cesium hydroxide: CsOH 
Calcium hydroxide: Ca(OH)2
Strontium hydroxide: Sr(OH)2
Barium hydroxide: Ba(OH)2
These bases completely dissociate in water. 

7. Acid/Base Strength vs. Concentration
Do not get acid/base strength confused with concentration.
Acid/base strength is based on the ability to dissociate.
Concentration is based on how much is dissolved in solution.
You can have a strong dilute acid – the acid completely dissociates, but there is not much acid dissolved in solution

8. Acid Ionization Constant
Acid ionization constant (Ka) is the value of the equilibrium constant expression(Keq) for the ionization of a weak acid.
Large Ka strong acid (much greater than 1)
Small Ka weak acid (much less than 1)

9. Base Ionization Constant
The base ionization constant (Kb) is the value of the equilibrium constant expression (Keq) for the ionization of a base
Large Kb strong base (much greater than 1)
Small Kb weak base (much less than 1)

10. Write the ionization equation and acid ionization constant (Ka) expressions for the acid HF
If you calculate Ka, it will be a weak acid so it will have a double arrow. Add it to water. HF(aq) + H2O(l)  H3O+(aq) + F- (aq) (A) (B) (CA) (CB)
Keq = Ka = [H3O+] [F -]
[HF]
Leave out liquids and solids in Keq
But keep products over reactants

11. Write the ionization equation and base ionization constant (Kb) expressions for the base NH3
If you calculate Kb, it will be a weak base so it will have a double arrow. Add it to water. NH3(aq) + H2O(l)  NH4+ (aq) + OH- (aq) (B) (A) (CA) (CB)
Keq = Kb = [NH4 +] [OH-]
[NH3]
Leave out liquids and solids in Keq
But keep products over reactants