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Answer :
Final answer:
The degree of dissociation of 0.01 M acetic acid in the presence of 0.01 M HCl can be calculated using the concept of equilibrium and the dissociation constant.
Explanation:
The dissociation constant of acetic acid at a given temperature is 1.69×10⁻⁵. The degree of dissociation of 0.01 M acetic acid in the presence of 0.01 M HCl can be calculated using the concept of equilibrium and the dissociation constant. In this case, the degree of dissociation would be equal to the concentration of the dissociated form of acetic acid divided by the initial concentration of acetic acid.
So, in this case, the degree of dissociation would be:
Degree of dissociation = [CH3COO-]/[CH3COOH]
Using the given dissociation constant of 1.69×10⁻⁵, we can calculate the degree of dissociation.
Therefore, the degree of dissociation of 0.01 M acetic acid in the presence of 0.01 M HCl would be 0.02 M * (1.69 × 10⁻⁵) = 0.000338.
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