Water has a molal freezing point constant of 1.86°C kg/mol.  Calculate the freezing point of 37.378 grams of calcium chloride (CaCl2) in 116.149 grams of water.  Assume complete dissociation.

At a certain temperature the vapor pressure of pure acetic acid (HCH₂CO₂) is measured to be 306. torr. Suppose a solution is prepared by mixing 127. g of acetic acid and 54.1 g of acetone ((CH3)₂CO). Calculate the partial pressure of acetic acid vapor above this solution. Round your answer to 3 significant digits. Note for advanced students: you may assume the solution is ideal. torr x10 ×

Complete combustion of 10.98 g of a compound of carbon, hydrogen, and oxygen yielded 16.10 g CO2 and 6.592 g H₂O. When 6.780 g of the compound was dissolved in 261 g of water, the freezing point of the solution was found to be -0.805 °C. For water, Kfp = 1.86 °C/m. What is the molecular formula of the compound? Enter the elements in the order C, H, O molecular formula =

The normal freezing point of a certain liquid X is 0.60°C, but when 0.14 kg of barium hydroxide (BaOH2) are dissolved in 900.g of X the solution freezes at −1.6°C instead. Use this information to calculate the molal freezing point depression constant Kf of X. Round your answer to 2 significant digits.

When 224. mg of a certain molecular compound X are dissolved in 45.0 g of cyclohexane (C6H₁2), the freezing point of the solution is measured to be 6.5 °C. Calculate the molar mass of X. If you need any additional information on cyclohexane, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 1 significant digit.

The freezing point of benzene, C6H6, is 5.500 °C at 1 atmosphere. Kf(benzene) = 5.12 °C/mIn a laboratory experiment, students synthesized a new compound and found that when 11.98 grams of the compound were dissolved in 212.6 grams of benzene, the solution began to freeze at 4.500 °C. The compound was also found to be nonvolatile and a non-electrolyte.What is the molecular weight they determined for this compound? ?g/mol

If 770 g of ethylene glycol (C2H6O2) is added to 1,000. g of water, what is the freezing point?    ° C

11. When 13.46 g of lactic acid, C3H6O3, are mixed with 119 g of stearic acid, the mixture freezes at 62.7 degrees C. The freezing point of pure stearic acid is 69.4 °C. What is the freezing point constant of stearic acid

A certain liquid  X  has a normal boiling point of  105.30°C  and a boiling point elevation constant  =Kb1.13·°C·kgmol−1 . Calculate the boiling point of a solution made of  52. g  of zinc chloride ( ZnCl2 ) dissolved in  450.g  of  X .

What would be the theoretical freezing point of a solution made by dissolving 5.052 g of CuCl 2 in 150.0 g of water? The freezing point constant of water is 1.86 °C/molal. The molar mass of CuCl 2 is 134.345 g/mol.     1.399 °C     -1.061 °C     -0.8277 °C     0.7148 °C     -1.399 °C