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The dissociation constant of acetic acid at a given temperature is [tex]1.69 \times 10^{-5}[/tex]. The degree of dissociation of 0.01 M acetic acid in the presence of 0.01 M [tex]\text{HCl}[/tex] is equal to:

Answer :

Final Answer:

The degree of dissociation of 0.01 M acetic acid in the presence of 0.01 M HCl is approximately 0.005.

Explanation:

Acetic acid (CH₃COOH) is a weak acid with a dissociation constant (Ka) of 1.69 x 10⁻⁵ at a given temperature. The degree of dissociation (α) represents the fraction of acid molecules that ionize in the solution.

In the presence of HCl, a strong acid, the equilibrium shifts towards complete ionization of HCl, leaving CH₃COOH primarily undissociated. Since acetic acid is weak, its dissociation is negligible compared to HCl. The concentration of H⁺ ions mainly comes from HCl.

Denoting the initial concentration of acetic acid as C₀ (0.01 M) and the degree of dissociation as α, the concentration of H⁺ ions from HCl is equal to the initial HCl concentration (0.01 M). The concentration of H⁺ ions from acetic acid (C₀ * α) is much smaller. As the strong acid dissociates almost completely, C₀ * α is negligible compared to 0.01 M.

Therefore, the practical degree of dissociation for acetic acid in the presence of 0.01 M HCl is approximately the same as without HCl, which is 1.69 x 10⁻⁵. Thus, the final answer is that the degree of dissociation is approximately 0.005.

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