A 3.782−g sample of a mixture of cyclohexane (C6H12) and naphthalene (C10H8) is dissolved in 57.30 g of benzene (C6H6). The freezing point of the solution is 1.90°C. Calculate the mass percent of the mixture. (See the table for constants.)  Solvent NormalBoiling Point Kb(°C/m) NormalFreezingPoint Kf (°C/m) Water 100 0.52 0.0 1.86 Benzene 80.1 2.53 5.5 5.12 Ethanol 78.4 1.22 −117.3 1.99 Acetic Acid 117.9 2.93 16.6 3.90 Cyclohexane 80.7 2.79 6.6 20.0 Naphthalene 80.6 6.9 208 5.95

When 225. g of alanine (C,H,NO₂) are dissolved in 1100. g of a certain mystery liquid X, the freezing point of the solution is 7.8 "C lower than the freezing point of pure X. On the other hand, when 225. g of ammonium chloride (NH,CI) are dissolved in the same mass of X, the freezing point of the solution is 21.8 °C lower than the freezing point of pure X. Calculate the van't Hoff factor for ammonium chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits.

A solution made by dissolving 150.0 g of an unknown compound in 375.0 mL of benzene to make a solution which has a freezing point 18.6 °C lower than that of pure benzene. Kf for benzene is 5.12 °C/m and the density of benzene is 0.877 g/mL. The molality of the solution is 3.63 m. What quantity in moles of the unknown compound were dissolved in the solution?

You are a forensic chemist and vou are given a white powder to analyze. You take a 0.25- g sample of this powder and dissolve it in 4.0 g of benzene. You determine that the freezing point of this solution is 3.9°C. Can you conclude that the compound is cocaine (C17H21NO4)? What assumptions did you make in the analysis?

A 12.7 g substance was dissolved in 2.00 g of solvent. The molar mass of the unknown substance is 169.7 g/mol. Calculate the freezing point depression. Kfof the substance = 6.0 K kg/mol.

Calculate the freezing point and boiling point for 0.43 molmol ethylene glycol and 0.17 mol KBrmol KBr in 124 gg H2OH2O.         Express your answer using one decimal place.

4. To make a solution, 40 g of a nonelectrolyte is dissolved into 300 g of water. The freezing point depression of the solution is measured to be -7°C. Calculate the molar mass of the solute. 5. In the commercial preparation of Hydrogen Chloride, what weight of HCl in grams may be obtained by heating 468 grams of NaCl with H,SO, 2Nacl + H,S04→ NaSO, + 2HCI

You dissolve a 30.0 g mixture of glucose (C₆H₁₂O₆) and NaCl in 1.00 kg water. The freezing point of this solution is found to be -0.765°C. Assuming ideal behavior, what is the mass (in grams) of glucose in the mixture? (Kf for water is 1.86°C･kg/mol).

Calculate the vapor pressure of a solution containing 28.5 g of glycerin (C3H8O3) in 125 mL of water at 30.0 degrees celsius. The vapor pressure of pure water at this temperature is 31.8 torr. Assume that glycerin is not volatile and dissolves molecularly (i.e. it is not ionic) and use a density of 1.00 g/mL for the water.

When 92.4 g of urea (CH₂N₂O) are dissolved in 1450. g of a certain mystery liquid X, the freezing point of the solution is 2.30 °C less than the freezing point of pure X. Calculate the mass of sodium chloride that must be dissolved in the same mass of X' to produce the same depression in freezing point. The van't Hoff factor -1.82 for sodium chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits. 0 0 8 alo X G V