If a 0.820 ? aqueous solution freezes at −2.70 ∘C, what is the van't Hoff factor, ?, of the solute?

A sample of an unknown compound with a mass of 0.546 g was dissolved in 15.0 g of benzene. The freezing point depression was measured as 0.240 oC. a) Calculate the molality of the solute. molality =

If a 0.690 ? aqueous solution freezes at −3.00 ∘C, what is the van't Hoff factor, ?, of the solute?

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 0.630 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 =

The ideal, theoretical, van't Hoff factor for SrCl, is 3, meaning it dissociates into 3 particles when dissolved in solution. An experiment was conducted to accurately determine the van't Hoff factor. A solution composed of 26.17 g of SrCl, was dissolved in to 475.0 mL of water at 285.2 K. The osmotic pressure was determined to be 23.04 bar. What is the experimental van't Hoff factor?

7.152g of an unknown solute was dissolved in 0.049883 kg of pure water. This solution has a boiling point of 103.4oC. The Van't Hoff factor of the unknown solute is 3. What is the Molality of the unknown? What is the Molecular weight of the unknown?

If a 0.580 m aqueous solution freezes at-2.30 °C, what is the van't Hoff factor, i, of the solute? Consult the table of K values.

A solution is made up of two volatile substances: liquid 1 for which P1*= 198 Torr and Liquid 2 for which P2* = 230 Torr. What is the molar mass of 8.824 kg of liquid 1, if the total vapor pressure is 215 Torr and there’s 2.00 total moles in solution.