1. Acids Lesson 3 Acid and Base Reactions

2. Conductivity The conductivity of an acid is determined by the number of ions generated in a solution and is therefore a combination of both the strength and concentration of the acid. 1.0 M HCl is a better conductor than 0.10 M HCl 1.0 M HI is a better conductor than 1.0 M HF. 1.0 M HF has the same conductivity as 0.02 M HCl.

3. Amphiprotic Chemical Species Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base. Acid, Base, or Amphiprotic PO 4 3-

4. Amphiprotic Chemical Species Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base. Acid, Base, or Amphiprotic PO 4 3- Basecan gain H +, cannot lose H + HPO 4 2-

5. Amphiprotic Chemical Species Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base. Acid, Base, or Amphiprotic PO 4 3- Basecan gain H +, cannot lose H + HPO 4 2- Amphiproticcan gain H + and lose H + H 2 PO 4 -

6. Amphiprotic Chemical Species Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base. Acid, Base, or Amphiprotic PO 4 3- Basecan gain H +, cannot lose H + HPO 4 2- Amphiproticcan gain H + and lose H + H 2 PO 4 - Amphiproticcan gain H + and lose H + H 3 PO 4

7. Amphiprotic Chemical Species Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base. Acid, Base, or Amphiprotic PO 4 3- Basecan gain H +, cannot lose H + HPO 4 2- Amphiproticcan gain H + and lose H + H 2 PO 4 - Amphiproticcan gain H + and lose H + H 3 PO 4 Acidcannot gain H +, can lose H +

8. Amphiprotic Chemical Species Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base. Acid, Base, or Amphiprotic CO 3 2-

9. Amphiprotic Chemical Species Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base. Acid, Base, or Amphiprotic CO 3 2- Base HCO 3 -

10. Amphiprotic Chemical Species Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base. Acid, Base, or Amphiprotic CO 3 2- Base HCO 3 - Amphiprotic H 2 CO 3

11. Amphiprotic Chemical Species Amphiprotic chemical species can act as acids and donate protons or bases and accept protons. They are listed both on the left side of the table as an acid and the right side as a base. Acid, Base, or Amphiprotic CO 3 2- Base HCO 3 - Amphiprotic H 2 CO 3 Acid

12. In Chemistry 11 H 2 SO 4 + 2KOH 

13. In Chemistry 11 H 2 SO 4 + 2KOH  K 2 SO 4 + 2HOH (l)

14. In Chemistry 11 H 2 SO 4 + 2KOH  K 2 SO 4 + 2HOH (l) 2H + + SO 4 2-

15. In Chemistry 11 H 2 SO 4 + 2KOH  K 2 SO 4 + 2HOH (l) 2H + + SO 4 2- + 2K + + 2OH - 

16. In Chemistry 11 H 2 SO 4 + 2KOH  K 2 SO 4 + 2HOH (l) 2H + + SO 4 2- + 2K + + 2OH -  2K + + SO 4 2- +

17. In Chemistry 11 H 2 SO 4 + 2KOH  K 2 SO 4 + 2HOH (l) 2H + + SO 4 2- + 2K + + 2OH -  2K + + SO 4 2- + 2HOH (l)

18. In Chemistry 11 H 2 SO 4 + 2KOH  K 2 SO 4 + 2HOH (l) 2H + + SO 4 2- + 2K + + 2OH -  2K + + SO 4 2- + 2HOH (l) H + + OH -  HOH (l) Use an arrow if you have a strong acid or a strong base! Strong acids, strong bases, and soluble salts are ionized!

19. In Chemistry 12 H 2 C 2 O 4 + 2KOH

20. In Chemistry 12 H 2 C 2 O 4 + 2KOH 

21. In Chemistry 12 H 2 C 2 O 4 + 2KOH  K 2 C 2 O 4 + 2HOH (l)

22. In Chemistry 12 H 2 C 2 O 4 + 2KOH  K 2 C 2 O 4 + 2HOH (l) H 2 C 2 O 4 + 2K + + 2OH -  2K + + C 2 O 4 2- + 2HOH (l)

23. In Chemistry 12 H 2 C 2 O 4 + 2KOH  K 2 C 2 O 4 + 2HOH (l) H 2 C 2 O 4 + 2K + + 2OH -  2K + + C 2 O 4 2- + 2HOH (l) H 2 C 2 O 4 + 2OH -  C 2 O 4 2- + 2HOH (l) The weak acid or base does not dissociate! Break up strong acids, strong bases, and soluble salts!

24. Conductivity Good ConductorsStrong AcidsStrong BasesSoluble Salts HClNaOHKCl Weak ConductorsWeak AcidsWeak BasesLow Solubility Salts HFZn(OH) 2 AgCl NonconductorsMolecular covalent C 12 H 22 O 11

25. In Chemistry 12 HC 2 O 4 - + HCO 3 - H+H+ The higher one on the acid side of the chart will be the acid and donate a proton. Weak acids and weak bases react but do not go to completion ( ⇋) ⇋ C 2 O 4 2- + H 2 CO 3 H+H+ BaseAcid Label all acids and bases- note H 2 C 2 O 4 donates in the reverse reaction The acid on the left HC 2 O 4 - is stronger than H 2 CO 3 so the other side or the products are favoured. AcidBase

26. ⇋ There are more products at equilibrium

27. The stronger acid H 2 SO 3 more successfully donates its proton making more reactants. Complete the reaction HSO 4 - + HSO 3 - ⇋ Reactants are Favoured because H 2 SO 3 is a stronger acid than HSO 4 - AcidBaseBase Acid SO 4 2- + H 2 SO 3 ⇋ H+H+ H+H+