The freezing point of benzene, C6H6, is 5.50 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in benzene is DDT. A student dissolves 11.78 grams of DDT, C14H9 C15 (354.5 g/mol), in 252.1 grams of benzene. Use the table of boiling and freezing point constants to answer the questions below. Solvent Water Ethanol Chloroform Benzene Formula H₂O CH3 CH₂ OH CHCl3 C6H6 Diethyl ether CH3 CH2 OCH2 CH3 The molality of the solution is The freezing point of the solution is Kb (°C/m) Kf (°C/m) 0.512 1.86 1.22 1.99 3.67 2.53 2.02 m. °C. 5.12

The boiling point of water is 100.0°C at 1 atmosphere. How many grams of silver acetate (166.9 g/mol), must be dissolved in 224.0 grams of water to raise the boiling point by 0.400 °C? mpor Refer to the table for the necessary boiling or freezing point constant. Solvent Kb (°C/m) Kf(°C/m) 0.512 1.22 Chloroform CHCl3 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH2 CH3 2.02 g silver acetate Water Ethanol Mass = this Formula H₂O CH3CH₂OH 1.86 1.99 5.12

The freezing point of water is 0.00°C at 1 atmosphere. How many grams of manganese(II) sulfate (151.0 g/mol), must be dissolved in 273.0 grams of water to reduce the freezing point by 0.350°C ? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kp (°C/m) Kf(°C/m) Water H20 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHC13 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH,CH3 2.02 g manganese(II) sulfate.

The freezing point of ethanol, CH3CH2OH, is -117.30°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is saccharin. A student dissolves 11.77 grams of saccharin, C,H;NO3S (183.2 g/mol), in 287.1 grams of ethanol. Use the table of boiling and freezing point constants to answer the questions below. Solvent Formula Kp (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH;CH2OH 1.22 1.99 Chloroform CHCI3 3.67 Benzene C,H6 2.53 5.12 Diethyl ether CH3CH,OCH2CH3 2.02 The molality of the solution is m. The freezing point of the solution is °C.

The freezing point of ethanol, CH3CH2OH, is -117.30°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is saccharin . A student dissolves 10.10 grams of saccharin, C7H5NO3S (183.2 g/mol), in 266.8 grams of ethanol. Use the table of boiling and freezing point constants to answer the questions below. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 X Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 X The molality of the solution is ______m.The freezing point of the solution is _____°C. FILL IN THE BLANKS

Consider naphthalene, C10H8. A solution of naphthalene is prepared by mixing 25.0g of naphthalene with 0.750 L of carbon disulfide CS2(density=1.263g/mL). Assume that the volume of the solution is the same as that of the solvent after the solution is prepared. The vapor pressure of pure CS2 at 25 degrees Celsius is 358 mm Hg. Calculate the vapor pressure of this solution at this temperature.

A solution is made by dissolving 7.80 grams of MgCl2 in 420.0 mL of water. What is the freezing point of this solution (in °C)? Express you answer to 3 significant digits.   Density of water 1.00 g/mL Kf of water 1.86oC/m

At 20°C, the vapor pressure of pure ethanol, C2H5OH, is 43.7 mmHg and the vapor pressure of pure n-propanol, C3H7OH, is 18.0 mmHg.What is the vapor pressure of a solution containing 50g of each alcohol?

The normal boiling point of a certain liquid X is 110.00 °C, but when 106. g of alanine (C3H,NO₂) are dissolved in 900. g of X the solution boils at 111.9 °C instead. Use this information to calculate the molal boiling point elevation constant K, of X. Round your answer to 2 significant digits. K₁=0 °C.kg mol X S

Determine the vapor pressure of a solution prepared by dissolving 16.8 mol of non-volatile aspirin (MM = 180.15 g/mol) in 0.691 kg of CH3CH2OH (MM = 46.07 g/mol) at 25 °C. Pº ethanol 44.0 torr at 25 °C. Give the answer to 3 significant figures. Do not include units. =