Question

Calculate the degree of dissociation of acetic acid (CH3COOH) given:

AmCctacoolD−11.7
Sim°CCH3COOH
40.9Scmmol−1
A°m(H₂O)349.1Scmmol−1


a. α=0.0013
b. α=0.0068
c. α=0.0031
d. α=0.0055

Answer 1

The degree of dissociation of acetic acid can be calculated using the given molar conductivity values and the equation α = (Λ - Λ0)/Λ0. Based on the calculations, the degree of dissociation is approximately 0.0031.

Step-by-step explanation:

The degree of dissociation, α, of acetic acid (CH3COOH) can be calculated using the equation α = [H+]/[CH3COOH]. In this case, we are given the molar conductivity of acetic acid (40.9 S cm^2 mol^-1) and the molar conductivity of water (349.1 S cm^2 mol^-1).

Using the molar conductivity of acetic acid and the molar conductivity of water, we can calculate the equivalent conductivity of the acetic acid solution, Λ, using the formula Λ = k * c, where k is the specific conductance of the solution and c is the concentration of the solution in mol L^-1.

Once we have Λ, we can calculate the degree of dissociation using the equation α = (Λ - Λ0)/Λ0, where Λ0 is the equivalent conductivity of the solution in the absence of dissociation.

For the given values, the calculated degree of dissociation is approximately 0.0031, so the correct answer is option c.