Acetic acid exists in benzene solution in the dimeric form. In an actual experiment the Van't Hoff factor of acetic acid in benzene solution was found to be 0.52. Calculate the degree of association and osmotic pressure of 0.1 M acetic acid solution in benzene at 300K

The degree of association (α) can be calculated using the formula:

α = 1 - (i / n)

Where: i = Van't Hoff factor n = number of particles the solute dissociates into

In this case, acetic acid exists as a dimer, so n = 2. The Van't Hoff factor i is given as 0.52.

Substituting these values into the formula, we get:

α = 1 - (0.52 / 2) α = 1 - 0.26 α = 0.74

So, the degree of association of acetic acid in benzene is 0.74 or 74%.

The osmotic pressure (π) can be calculated using the formula:

π = iCRT

Where: C = molar concentration of the solute R = universal gas constant (0.0821 L atm / mol K) T = absolute temperature in Kelvin

Substituting the given values into the formula, we get:

π = 0.52 * 0.1 * 0.0821 * 300 π = 1.28 atm

So, the osmotic pressure of the solution is 1.28 atm.