The boiling point of pure ethanol (C₂H5OH, MM = 46.07 g/mol) is 78.4 °C. A solution is made using 100.0 g of ethanol (the solvent) and 12.1 g of glucose (MM = 180.16 g/mol). What is the boiling point of this solution, in °C? (Kb of ethanol is 1.22 °C/m)

The freezing point of water is 0.00°C at 1 atmosphere. A student dissolves 13.21 grams of sodium chloride, NaCl (58.40 g/mol), in 282.7 grams of water. 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 CH;CH2OH 1.22 1.99 Chloroform CHC13 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH,OCH,CH3 2.02 The molality of the solution is m. The freezing point of the solution is °C.

Insulin is a protein that regulates carbohydrate metabolism by decreasing blood sugar levels. A deficiency in insulin leads to diabetes. An aqueous solution of insulin contains 0.360 moles of insulin in 50.0 g water. What is the boiling point of this solution? Water has a kb = 0.512 °C/m and the molar mass of insulin is 5730 g/mol.

A certain liquid X has a normal boiling point of 129.10 °C and a boiling point elevation constant K₁=0.95 °C-kg-mol¯¹. Calculate the boiling point of a solution made of 58.g of benzamide (C₂H₁NO) dissolved in 400. g of X. Round your answer to 4 significant digits. [°C x10 X Ś

The boiling point of pure ethanol is 78.4 °C. A solution is made using 100.0 g of ethanol (the solvent) (MM = 46.07 g/mol) and 20.1 g of methanol (MM = 32.04 g/mol). What is the boiling point of this solution? (Kb of ethanol is 1.22 °C/m)

A 83.5 g sample of a nonelectrolyte is dissolved in 250.1 g of water. The solution is determined to have a boiling point of 102.3 °C. What is the molar mass of the compound? (Kb for water is 0.510 °C/m).

A certain liquid X has a normal boiling point of 117.90 °C and a boiling point elevation constant K,= 1.09 °C·kg'mol Calculate the boiling point of a solution made of 95.g of sodium chloride (NaCl) dissolved in 900. g of X. Round you answer to 4 significant digits.

What is the boiling point of a solution prepared by dissolving 37.5 g of glucose (C6H12O6, MW=180.16g/mol) in 750 g of ethanol (CH3CH2OH, MW=46.07g/mol)? Kb 1.22°C/m, boiling point of pure ethanol=78.24°C? ATb=ikbm 78.56°C 70.57°C 77.91°C 85.91°C

At a certain temperature the vapor pressure of pure water is measured to be 233. mmHg. Suppose a solution is prepared by mixing 131. g of water and 71.8 g of acetic acid (HCH,CO2). Calculate the partial pressure of water vapor above this solution. Round your answer to 3 significant digits. Note for advanced students: you may assume the solution is ideal. | mmHg x10

How many grams of glucose (molar mass = 180.16 g mol1) must be dissolved in 255 g of water to raise the boiling point to 102.56 °C? Mass of glucose = g Use correct number of significant digits;