How can compare the moles of acetic acid molecules

Question

The molal freezing point depression constant of benzene K_f= 5.09^oCkg/mole. Benzene, C₆H₆, a common non-polar organic solvent, is neither acidic nor basic, and can neither donate nor accept hydrogen bonds.  On a certain thermometer, the freezing point of pure liquid benzene was measured as +5.50^oC. How can compare the moles of acetic acid molecules in the 3.74g of the acetic acid itself to the moles of solute particles when that much acetic acid is dissolved in the benzene? Does acetic acid dissociate, or does it behave as intact single molecules, or does it associates when dissolved in benzene when a solution of 3.74g of acetic acid, CH₃COOH, in 100g of benzene froze at +3.87^oC measured on the same thermometer.