1. 10.1 Acid – Base Theories
Ms. Munir

3. Properties of Acids and Bases
Acids can be distinguished from bases via their physical properties:
acids taste sour; they change colour when mixed with indicators.
Bases taste bitter & feel slippery; they change colour when mixed with indicators.

9. The Arrhenius Theory of Acids and Bases
Ions are present in solutions of acids and bases.
When HCl dissolves in water, it dissociates into H+ ions and Cl- ions.
HCl(aq) → H+(aq) + Cl−(aq)
When NaOH dissolves in water, it dissociates into Na+ ions and OH− ions.
NaOH(aq) → Na+(aq) + OH−(aq)

11. Theory The Arrhenius theory of acids and bases states that:
An acid is a substance that dissociates in water to produce one or more hydrogen ions, H+.
A base is a substance that dissociates in water to form one or more hydroxide ions, OH−.

12. Limitations of the Arrhenius Theory
Consider:
HCl(aq) → H+(aq) + Cl−(aq)
This dissociation occurs in aqueous solution, but H2O is left out as a component of the reaction. It is assumed to be there. Put H2O into the equation:
HCl(aq) + H2O(l) → H+(aq) + Cl−(aq) + H2O(l)
Water is unchanged in this reaction.

13. Water is a polar molecule.
The O atom has a partial -ve charge, and the H atoms have partial +ve charges. So, H2O must interact with the ions H+ and Cl−.
Protons (H+ ions) do not exist in isolation in aqueous solution.
Protons are always hydrated: they are attached to water molecules. A hydrated proton is called a hydronium ion, H3O+(aq).

14. NH3(g) + H2O(l) → NH+4(aq) + OH−(aq)
Consider:
NH3(g) + H2O(l) → NH+4(aq) + OH−(aq)
Ammonia is one of several substances that produce basic solutions in water.
Ammonia does not contain hydroxide ions.
It does produce these ions when it reacts with water.

15. The Arrhenius theory can’t explain the basic properties of ammonia
The Arrhenius theory can’t explain the basic properties of ammonia. Nor can it explain the fact that certain other substances, such as salts that contain carbonate ions, also have basic properties.
Arrhenius theory is limited to acid-base reactions in a single solvent, water. Many acid-base reactions take place in other solvents also.

16. The Brønsted-Lowry Theory of Acids and Bases
An acid is a substance from which a proton (H+ ion) can be removed.
A base is a substance that can remove a proton (H+ ion) from an acid.

17. Explanation A Brønsted-Lowry acid must contain H in its formula.
All Arrhenius acids are also Brønsted-Lowry acids.
Any -ve ion (not just OH−) can be a Brønsted-Lowry base.
Water is not the only solvent that can be used.

18. According to the Brønsted-Lowry theory, an acid base reaction involves the transfer of a proton.

19. Example
Consider the reaction between HCl acid and H2O. Here, HCl is an acid because it provides a proton (H+) to the water. The water molecule receives the proton. Therefore, according to the Brønsted-Lowry theory, water is a base in this reaction. When the water receives the proton, it becomes a hydronium ion (H3O+).

20. Conjugate acid and base
Two molecules or ions that are related by the transfer of a proton are called a conjugate acid-base pair.
The conjugate base of an acid is the particle that remains when a proton is removed from the acid. The conjugate acid of a base is the particle that results when the base receives the proton from the acid.

21. Example
Hydrogen bromide is a gas at room temperature. It is soluble in water, forming hydrobromic acid. Identify the conjugate acid-base pairs.

22. Solution

23. Example
Identify the conjugate acid-base pairs in the reaction between ammonia and water.

24. Solution

25. Homework P 379-380 # 1 – 10 McGrawHill
No work from Nelson; use McGrawHill