Free Version
Difficult

# Determining Equilibrium Constant from Freezing Point Depression

CHEM-XPROEH

The compound acetic acid undergoes dimerization in solution by the following reaction:

When $3.76 \textrm{ g}$ of acetic acid is dissolved in $100.0 \textrm{ g}$ of benzene, the freezing point is lowered by $1.66 °\textrm{C}$.

The density of the equilibrium mixture is $0.9067 \frac{\textrm{g}}{\textrm{mL}}$ and molal freezing-point depression constant for benzene is $K_f = -5.12 \frac{°\textrm{C kg}}{\textrm{mol}}$.

What is the value of the equilibrium constant, $K$, for the dimerization of acetic acid in solution at this temperature?

A

6.19

B

151

C

592

D

605

E

667