1. Strong vs Weak Acids
201 Chemistry

2. NaCl(s) Na+(aq) + Cl-(aq)
Dissociation
Dissociation (ionisation) is when an ionic solid breaks up into its ions when in solution
NaCl(s) Na+(aq) + Cl-(aq)

3. HCl(g) + H2O(l) H3O+(aq) + Cl-(aq)
Strong Acids
Readily donate protons
Become fully dissociated
HCl(g) + H2O(l) H3O+(aq) + Cl-(aq)
Solution contains, H2O molecules, H3O+ and Cl- ions and no HCl molecules

5. CH3COOH(aq) + H2O(l) CH3COO-(aq) + H3O+(aq)
Weak Acids
Limited proton donation
Only partially dissociates
CH3COOH(aq) + H2O(l) CH3COO-(aq) + H3O+(aq)
Solution contains mostly H2O and CH3COOH molecules and only a few CH3COO- and H3O+ ions

7. NaOH(s) Na+(aq) + OH-(aq)
Strong Bases
Readily accepts protons
Becomes completely dissociated
NaOH(s) Na+(aq) + OH-(aq)

8. NH3(aq) + H2O(l) NH4+(aq) + OH-(aq)
Weak Bases
Limited proton accepting
Only partially dissociates
NH3(aq) + H2O(l) NH4+(aq) + OH-(aq)

9. Dilute & Concentration
Concentrated acids contain more H3O+ ions
Concentrated bases contain more OH- ions

10. Concentration vs Strength
Concentration refers to amount H3O+/OH- ions at a given volume.
Strength refers to the ease a substance will undergo proton transfer

11. Conductivity
Strong acids fully dissociate into charged ions therefore are excellent conductors of electricity
HA(g) + H2O(l) → H3O+(aq) + A-(aq)
Weak acids are only partially dissociated therefore are poor conductors of electricity
HA1(aq) + H2O(l) ↔ H3O+(aq) + A1-(aq)

12. pH
Weak acids have a higher pH than strong acids of the same concentration as the actual concentration of H3O+ is less.
This is because most of the acid remains in the molecular form.

13. Rate of Reaction
Strong acids fully dissociate therefore there is a higher concentration of H3O+ ions which leads to a faster rate of reaction
HA(g) + H2O(l) → H3O+(aq) + A-(aq)
Weak acids are only partially dissociated most of the acid remains in its molecular form. There is a lower concentration of H3O+ ions so a slower rate of reaction
HA1(aq) + H2O(l) ↔ H3O+(aq) + A-(aq)

14. HA(aq) + H2O(l) ↔ H3O+(aq) + A-(aq)
Extent of Reaction
Even though weak acids are only partially dissociate it is in equilibrium.
As a reaction proceeds (the H3O+ is used/removed) the equilibrium favours the forwards reaction and more h3o+ is made. The reaction continues until either the acid or other reactant is used up.
HA(aq) + H2O(l) ↔ H3O+(aq) + A-(aq)