Solutions Quiz-4

A solution containing 1.8g of a compound (empirical formula $CH_2O$) in 40g of water is observed to freeze at $-0.465^\circ C$. The molecular formula of the compound is ($K_f = 1.86\text{ kg K mol}^{-1}$)

$K_f$ for water is $1.86\text{ K kg mol}^{-1}$. If your automobile radiator holds 1.0 kg of water, how many grams of ethylene glycol ($C_2H_6O_2$) must you add to get the freezing point of the solution lowered by $2.8^\circ C$?

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

The freezing point of water is depressed by $0.37^\circ C$ 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 $1.86^\circ C\,m$. If 5.00 g of $Na_2SO_4$ is dissolved in 45.0g of $H_2O$, the freezing point is found to be $-3.82^\circ C$. Calculate the can’t Hoff factor for $Na_2SO_4$.

0.01 M solution of KCl and $BaCl_2$ are prepared in water. The freezing point of KCl solution is fount to be$-2^\circ C$. What is the freezing point of $BaCl_2$ 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 $\pi$, what will be the osmotic pressure for 0.1 M NaCl?

An aqueous solution containing 1.248g of barium chloride (molar mass = 208.34g $mol^{-1}$) in 100g of water boils at $100.0832^{\circ} C$. Calculate the degree of dissociation of $BaCl_2$ ($K_f$ for water$= 0.52\text{ K kg mol}^{-1}$)

The Henry’s law constant for the solubility of $N_2$ gas in water at 298 K is $1.0 \times 10^{5}$ atm. The mole fraction of $N_2$ in air is 0.8. The number of moles of $N_2$ from air dissolved in 10 moles of water at 298 K and 5 atm pressure is.