1. Strong vs Weak Acids/Bases
Strong acids or bases dissociate completely while weaker acids and bases only partially dissociate.

2. Strong vs Weak Acid Strong Acid:
HCl (aq)  H+ (aq) + Cl- (aq) Exists only in the form of ions
HCl + H2O  H3O Cl- The actual ion species
(Lots of H3O+ )
Weak Acid:
CH3COOH (acetic acid-vinegar is 4-18% acetic acid by mass)
CH3COOH H2O  H3O CH3COO-
(Little of H3O+)
Most of the aa is in the combined form to the left of 

3. Experimental Evidence for Strong vs Weak Acids
Solutions with many charged ions will conduct electricity better which can be measured with a qualitative (showing a general change) or quantitative (giving exact numbers) device. The conductivity device shown shows qualitative differences.
strong acid weak acid

4. The Organic Acid Group
In the COOH group, the doubly bonded oxygen and the other oxygen exert a strong pull on the hydrogen’s electron. Under the right circumstances, this causes the hydrogen proton to leave its electron with the group and split off as a hydrogen ion which then attaches to a water molecule to form a hydronium ion.
CH3COOH H2O  CH3COO H3O+

5. Dilute/Concentrated - Not the same as Weak/Strong
Dilute and concentrated refers to the molarity of a solution (particles of acid/base per volume of solution).
Weak vs Strong refers to the % ionization of an acid/base.
A 10.0 M HF (aq) solution is CONCENTRATED but WEAK.
A .001 M HCl (aq) solution is DILUTE but STRONG
A 10.0 M HF(aq) solution actually has less H3O+ than a
.1M HCl(aq) solution even though it is 100X more concentrated – because it is much less ionized.

6. Using the Table of Relative Strengths of Acids and Bases

7. Using the Table of Relative Strengths of Acids and Bases

8. Neutral Water’s Ionization
H2O + H2O kJ  H3O+ (aq) + OH- (aq) at 25o C

9. Water’s Ionization Constant
H2O + H2O kJ  H3O+ (aq) + OH- (aq) at 25o C
Kw = [H3O][OH-] = 1 x 10-14
[H3O] = 1 x 10-7
[OH-] = 1 x 10-7
Note that with neutral water at 25o C, the concentrations of H3O+ and OH- are equal.

10. Water’s [H3O+] Over 25o C
H2O + H2O kJ  H3O+ (aq) + OH- (aq) at 25o C
At temperatures above 25 C, the equilibrium shifts right.
This produces more [H3O+] and [OH-].
More [H3O+] typically means greater acidity but not here.
Since the [H3O+] = [OH-] , the water is still neutral (although its pH drops due to the extra hydronium [H3O+] ions).

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