A solution containing 1.8g of a compound (empirical formula $C{H}_{2}OCH\_2O$) in 40g of water is observed to freeze at $-0.465^{\circ }C-0.465^\backslash circ\; C$. The molecular formula of the compound is ($K_f=1.86{\text{ kg K mol}}^{-1}K\_f\; =\; 1.86\backslash text\{\; kg\; K\; mol\}^\{-1\}$)

$K_{f}K\_f$ for water is $1.86{\text{ K kg mol}}^{-1}1.86\backslash text\{\; K\; kg\; mol\}^\{-1\}$. If your automobile radiator holds 1.0 kg of water, how many grams of ethylene glycol ($C_2{H}_6{O}_{2}C\_2H\_6O\_2$) must you add to get the freezing point of the solution lowered by $2.8^{\circ }C2.8^\backslash circ\; C$?

Calculate the molal depression constant of a solvent which has freezing point $16.6^{\circ }C16.6^\backslash circ\; C$ and latent heat of fusion $180.75J{g}^{-1}\mathrm{.}180.75\backslash ,\; J\backslash ,\; g^\{-1\}.$.

The freezing point of water is depressed by $0.37^{\circ }C0.37^\backslash circ\; C$ in a 0.01 molal NaCl solution. The freezing point of 0.02 molal solution of urea is depressed by.

The freezing point depression constant of water is $1.86^{\circ }Cm1.86^\backslash circ\; C\backslash ,m$. If 5.00 g of $N{a}_{2}S{O}_{4}Na\_2SO\_4$ is dissolved in 45.0g of $H_{2}OH\_2O$, the freezing point is found to be $-3.82^{\circ }C-3.82^\backslash circ\; C$. Calculate the can’t Hoff factor for $N{a}_{2}S{O}_{4}Na\_2SO\_4$.

0.01 M solution of KCl and $BaC{l}_{2}BaCl\_2$ are prepared in water. The freezing point of KCl solution is fount to be$-2^{\circ }C-2^\backslash circ\; C$. What is the freezing point of $BaC{l}_{2}BaCl\_2$ solution, assuming complete Ionization?

Van't Hoff factors of aqueous solution of X, Y and Z are 1.8, 0.8 and 2.5 respectively. Hence, correct order of the colligative property will be?

If osmotic pressure of 1 M urea is $\pi \backslash pi$, what will be the osmotic pressure for 0.1 M NaCl?

An aqueous solution containing 1.248g of barium chloride (molar mass = 208.34g $mo{l}^{-1}mol^\{-1\}$) in 100g of water boils at $100.0832^{\circ }C100.0832^\{\backslash circ\}\; C$. Calculate the degree of dissociation of $BaC{l}_{2}BaCl\_2$ ($K_{f}K\_f$ for water$=0.52{\text{ K kg mol}}^{-1}=\; 0.52\backslash text\{\; K\; kg\; mol\}^\{-1\}$)

The Henry’s law constant for the solubility of $N_{2}N\_2$ gas in water at 298 K is $1.0\times 10^{5}1.0\; \backslash times\; 10^\{5\}$ atm. The mole fraction of $N_{2}N\_2$ in air is 0.8. The number of moles of $N_{2}N\_2$ from air dissolved in 10 moles of water at 298 K and 5 atm pressure is.