When 40.3 g of urea (CH₂N₂O) freezing point of pure X. are dissolved in 750. g of a certain mystery liquid X, the freezing point of the Calculate the mass of ammonium chloride (NH₂CI) that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't Hoff factor i=1.60 for ammonium chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits.

Menthol is a crystalline substance with a peppermint taste and odor. When 1.10g of menthol is dissolved in 25.0 g of cyclohexane, the freezing point of the solution is lowered by 5.87 °C. The freezing point and Kf constant for cyclohexane can be found here. Calculate the molar mass of menthol.

The freezing point of 57.08 g of a pure solvent is measured to be 50.83 ºC. When 2.86 g of an unknown solute (assume the van 't Hoff factor = 1.0000) is added to the solvent the freezing point is measured to be 48.78 ºC. Answer the following questions ( the freezing point depression constant of the pure solvent is 7.33 ºC·kg solvent/mol solute). Be sure to use the appropriate number of sig figs What is the molality of the solution?  How many moles of solute are present?   What is the molecular weight of the solute?

A solution of 4.55 % phenol (C6H6O) solution by mass in carbon tetrachloride, CCl4.  The density of the solution is 1.602g/mL.  What are the molality, mole fraction, and molarity of phenol in the solution?   a. Fill in the summary table as you determine different parts of the problem – the first few columns are labeled – it is up to you to decide what is important information:   Molar mass mole         Solute             Solvent             Solution               b. Molality:   c. Mole Fraction:     d. Molarity: