If a 0.900 m aqueous solution freezes at -2.00 Celsius, what is the van't Hoff factor, i, of the solute?

An ionic compound is found to have a molar mass of 245 g/mol with the Van't Hoff factor (i) 2.  If 56 mg of the compound is dissolved in enough water to make 310 mL of solution at 28°C, what is the osmotic pressure (in torr) of the resulting solution? Assume that the compound is a molecular system. 1atm = 760 torr.

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FeCl₃ has a van't Hoff factor of i = 3.40. What is the concentration of particles in a 0.501 M solution of FeCl₃?

What is the mole fraction, X, of solute and the molality, m (or b), for an aqueous solution that is 14.0% NaOH by mass? X = m = m

If a 0.570 m aqueous solution freezes at -2.90 °C, what is the van't Hoff factor, i, of the solute? Consult the table of Kf values. i =

If a 0.630 m aqueous solution freezes at -2.00 °C, what is the van't Hoff factor, i, of the solute? Consult the table of Kf values. i =

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Calculate the vapor pressure (in torr) at 298 K in a solution prepared by dissolving 12.32 g of the non-volatile non-electrolye urea {CO(NH2)2} in 154 g of water. The vapor pressure of water at 298 K is 23.76 torr.   Enter your answer to 2 decimal places.

What is the mole fraction of 25% sucrose solution (C 12 H 22 O 11 )? Find its molality.