1. Acids Lesson 4 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. The same is true for a base. 0.004 M NaOH has the same conductivity as 1.0 M NH 3

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.

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-

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-

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 -

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

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 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 +

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-

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 -

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

12. 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

13. In Chemistry 11 H 2 SO 4 + 2KOH 

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

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

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

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- +

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)

19. 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!

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 Weak acids and weak bases also react. Use ⇋ Do not go to completion.

26. In Chemistry 12 Weak acids and weak bases also react. Use ⇋ Do not go to completion. HC 2 O 4 - + HCO 3 - ⇋

27. In Chemistry 12 Weak acids and weak bases also react. Use ⇋ Do not go to completion. HC 2 O 4 - + HCO 3 - ⇋ Look up the two amphiprotic ions on the left side of the acid chart. The higher one is the stronger acid and will be the acid and donate a proton to the base.

28. In Chemistry 12 Weak acids and weak bases also react. Use ⇋ Do not go to completion. HC 2 O 4 - + HCO 3 - ⇋ AcidBase Look up the two amphiprotic ions on the left side of the acid chart. The higher one is the stronger acid and will be the acid and donate a proton to the base. H+H+

29. In Chemistry 12 Weak acids and weak bases also react. Use ⇋ Do not go to completion. HC 2 O 4 - + HCO 3 - ⇋ C 2 O 4 2- + H 2 CO 3 AcidBase

30. In Chemistry 12 Weak acids and weak bases also react. Use ⇋ Do not go to completion. HC 2 O 4 - + HCO 3 - ⇋ C 2 O 4 2- + H 2 CO 3 AcidBase Label the acid and base on the other side of the equation. You do this by considering which species will donate the proton in the reverse reaction.

31. In Chemistry 12 Weak acids and weak bases also react. Use ⇋ Do not go to completion. HC 2 O 4 - + HCO 3 - ⇋ C 2 O 4 2- + H 2 CO 3 AcidBase Label the acid and base on the other side of the equation. You do this by considering which species will donate the proton in the reverse reaction. H+H+

32. In Chemistry 12 Weak acids and weak bases also react. Use ⇋ Do not go to completion. HC 2 O 4 - + HCO 3 - ⇋ C 2 O 4 2- + H 2 CO 3 AcidBaseBaseAcid H+H+

33. In Chemistry 12 Weak acids and weak bases also react. Use ⇋ Do not go to completion. HC 2 O 4 - + HCO 3 - ⇋ C 2 O 4 2- + H 2 CO 3 AcidBaseBaseAcid Now compare the acid on the left HC 2 O 4 - to the acid on the right H 2 CO 3. HC 2 O 4 - is the stronger acid and more successfully donates its proton to favour the formation of products. This means there are more products than reactants at equilibrium. When you find the stronger acid, the other side is always favoured.

34. In Chemistry 12 Weak acids and weak bases also react. Use ⇋ Do not go to completion. HC 2 O 4 - + HCO 3 - ⇋ C 2 O 4 2- + H 2 CO 3 AcidBaseBaseAcid Stronger acid Products are favoured! ⇋

35. In Chemistry 12 HSO 4 - + HSO 3 - ⇋

36. In Chemistry 12 HSO 4 - + HSO 3 - ⇋ HSO 4 - is a stronger acid than HSO 3 - so it donates the proton.

37. In Chemistry 12 HSO 4 - + HSO 3 - ⇋ SO 4 2- + H 2 SO 3 AcidBase

38. The stronger acid H 2 SO 3 more successfully donates its proton making more reactants. In Chemistry 12 HSO 4 - + HSO 3 - ⇋ SO 4 2- + H 2 SO 3 AcidBaseBaseAcid Reactants are Favoured because H 2 SO 3 is a stronger acid than HSO 4 - H+H+ ⇋