2. Which of the following acids is the strongest and which one is the weakest. Explain.
Thus, larger the Ka value stronger is the acid. Therefore,
3. Calculate the degree of ionization and [H3O+] of a 0.1 mol /L solution of acetic acid. Given: Ka(CH3COOH) = 1.8 x 10-5 mol / L.
Let 'a' be the degree of ionization. The concentration of various species involved in the equilibrium are as follows:
The equilibrium constant for the ionization of CH3COOH can be written as follows:
CH3COOH is very feebly ionized. So, 'a' may be ignored in comparison to 1. Then,
4. At 298 K, a 0.1 M solution of acetic acid is 1.34% ionized. What is the ionization constant (Ka) for the acid?
Acetic acid ionizes as follows: