Write the value of the van't Hoff factor $(i)$ for $K_{2}SO_{4}$ and $K_{4}[Fe(CN)_{6}]$.

What is the freezing point (in $^\circ C$) of a solution containing $0.1 \ g$ of $K_3[Fe(CN)_6]$ (molar mass = $329 \ g \ mol^{-1}$) in $100 \ g$ of water? (Given $K_f = 1.86 \ K \ kg \ mol^{-1}$)

For a dilute aqueous solution of glucose,the van't Hoff factor $(i)$ is:

Which of the following has the lowest freezing point?

$19.5 \text{ g}$ of fluoroacetic acid (molar mass = $78 \text{ g mol}^{-1}$) is dissolved in $500 \text{ g}$ of water at $298 \text{ K}$. The depression in the freezing point of water was $1^\circ\text{C}$. What is $K_a$ of fluoroacetic acid? (For water, $K_f = 1.86 \text{ K kg mol}^{-1}$). Assume molarity and molality to have same values.

For very dilute solutions of $BaCl_2$ $(t_1)$ and $KCl$ $(t_2)$ having the same molarity,what is the correct relationship between their boiling points?