1. Acids and Bases

2. Characteristics:

3. Characteristics: … +

4. Characteristics: … +

5. AMPHIPROTIC vs AMPHOTERIC SUBSTANCES
AMPHIPROTIC DEF: Substance that can both lose and gain a proton, relevant to the same solid.
AMPHOTERIC DEF:
Can behave as both an acid and a base.

6. PROTON TRANSFER EQUILIBRIA IN WATER
When a species donates a proton, it becomes the conjugate base; when a species gains a proton, it becomes the conjugate acid. Conjugate acids and bases are in equilibrium in solution.
The strength of a Brønsted acid is measured by its acidity constant, and the strength of a Brønsted base is measured by its basicity constant; the stronger the base, the weaker is its conjugate acid.
Base 1 = conjugate base of Acid 1.
Acid 2 = conjugate acid of Base 2.
The conjugate base of an acid is the species that is left after a proton is lost.
The conjugate acid of a base is the species formed when a proton is gained.

7. ELECTROLYTE STRENGTH

10. MEASUREMENTS & pH SCALE

11. TITRATION:
- Experimental procedure by which acids and bases are reacted, most commonly for purposes of quantitative analysis

13. Equilibrium in Bronsted Acid-Base Systems

14. Equilibrium in Bronsted Acid-Base Systems

15. How do we know what the end point is pH the indicator will change colour?

16. Van’t Hoff Equation:

17. Mixture of a strong acid with a strong base:

18. Polyprotic Acids -Can furnish more than one proton/molecule
-Always dissociates in a step wise manner, one proton at a time

19. QUESTIONS:
1. Identify the conjugate bases corresponding to the following acids: [Co(NH3)5(OH2)]3+, HSO4–, CH3OH, H2PO4–, Si(OH)4, HS–. Also write the acid-base reaction with water for each acid and label the acid, base, and conjugate acid.
2. Write the expression for Ka for each reaction.
- HCO−3(aq)+H2O(l)⇌CO2−3(aq)+H3O+(aq)
- formicacid(aq)+H2O(l)⇌formate(aq)+H3O+(aq)
- H3PO4(aq)+H2O(l)⇌H2PO−4(aq)+H3O+(aq)

20. QUESTIONS:
3. Show that water is amphiprotic by writing balanced chemical equations for the reactions of water with HNO3 and NH3 . In which reaction does water act as the acid? In which does it act as the base?
4. Calculate the pH and the pOH of each solution.
a) MHBr
b) MKOH
c) 2.3×10−3MHNO3
d) 9.78×10−2MNaOH

21. QUESTIONS: 5. Calculate the pH and the pOH of each solution.
a) 25.0 mL of 2.3×10−2MHCl , diluted to 100 mL
b) 5.0 mL of 1.87MNaOH , diluted to 125 mL
c) 5.0 mL of 5.98MHCl added to 100 mL of water