The freezing point of water is 0.00 °C at 1 atmosphere. How many grams of aluminum sulfate (342.2 g/mol), must be dissolved in 242.0 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 Water H₂O Ethanol CH3 CH₂ OH Chloroform CHCl3 Benzene C6H6 Diethyl ether Formula Mass= Kb (°C/m) Kf(°C/m) 0.512 1.22 3.67 g 2.53 CH3 CH₂ OCH₂ CH3 2.02 1.86 1.99 5.12

[References] Use the References to access important values if needed for this question. The boiling point of ethanol, CH3 CH₂OH, is 78.500 °C at 1 atmosphere. K₁ (ethanol) = 1.22 °C/m In a laboratory experiment, students synthesized a new compound and found that when 14.95 grams of the compound were dissolved in 293.3 grams of ethanol, the solution began to boll at 78.570 °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 Submit Answer Retry Entire Group 9 more group attempts remaining Show Hint Congage Learning Cengage Technical Support Previous Next Save and Exit

When 0.52 g of an unknown nonelectrolyte are dissolved in 35.0 g cyclohexane, the freezing point of the solution is 5.1ºC.  Pure cyclohexane freezes at 6.6ºC and has a Kf of 20.0ºC/m. What is the molar mass of the unknown in g/mol? Enter your answer with no decimal places (round to the nearest whole number). Do not include units. Do not worry about significant figures. Example: 2

-1 A certain liquid X has a normal freezing point of 5.90 °C and a freezing point depression constant K,=5.86 °C·kg•mol . Calculate the freezing point of a solution made of 20.1g of barium hydroxide (Ba(OH),) dissolved in 250. g of X. Round your answer to 3 significant digits. °C x10