Ka for ch3coh is 1.8x10^-5. Find out percentage dissociation of 0.2M CH3COOH in 0.1M HCl solution.
To find out the percentage dissociation of CH3COOH in an HCl solution, we need to use the equilibrium constant (Ka) for the dissociation reaction.
First, let's write the dissociation reaction for CH3COOH:
CH3COOH ⇌ CH3COO- + H+
Given that the Ka for CH3COOH is 1.8x10^-5, we can use this value to calculate the degree of dissociation (α) for CH3COOH.
The formula for α is: α = √(Ka * C), where C is the initial concentration of CH3COOH.
In this case, the initial concentration of CH3COOH is 0.2 M. Therefore, we calculate α as follows:
α = √(1.8x10^-5 * 0.2)
α ≈ 0.001897
The degree of dissociation (α) represents the fraction of CH3COOH that dissociates into CH3COO- and H+. To find the percentage dissociation, we need to multiply α by 100:
Percentage dissociation = α * 100
Percentage dissociation ≈ 0.001897 * 100
Percentage dissociation ≈ 0.1897%
Therefore, the percentage dissociation of 0.2 M CH3COOH in a 0.1 M HCl solution is approximately 0.1897%.