Calculate the freezing and boiling point of a solution containing 10.0g of naphthalene (C10H3) in 100.0mL of benzene ( CHs). Benzene has a density of 0.877g/cm3. Benzene boils and freezes at 80.1 °C and 5.5°C respectively. The Kb for benzene is 2.53 °C/m and Kf is 5.5 °C/m.

An aqueous solution of a molecular compound boils at 114.5°C. What is the molality, m, of the solution? The Kb=0.512°C/m for water and its boiling point is 100.0 °C. Express your answer to two decimal positions.

Select the one with the highest boiling point. Select the one with the lowest freezing point. A. 1.0 m KNO3 B. 0.75 m NaCl C. 0.75 m CuCl₂ D. 2.0 m C12H22O11 (sucrose) E. pure water Determine the freezing point of a solution that contains 0.31 mol of sucrose in 175 g of water, where K₁ = 1.86°C/m. A. 3.3°C Your answer: B. 1.1°C C. 0.0°C D. -1.1°C E. -3.3°C

The boiling point of pure ethanol (C₂H-OH, MM = 46.07 g/mol) is 78.4 °C. A solution is made using 100.0 g of ethanol (the solvent) and 24.1 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) 1 4 7 +/-

9. Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H602) dissolved in 500.0 g of water. K/= 1.86°C/m and Kb = 0.512°C/m. Use 100°C as the boiling point of water.

The freezing point of water is 0.00°C at 1 atmosphere.A student dissolves 12.66 grams of chromium(II) acetate, Cr(CH3COO)2 (170.1 g/mol), in 281.4 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 CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67   Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02   The molality of the solution is  ?The freezing point of the solution is  ?

Calculate the boiling point of a solution of 400 g of ethylene glycol dissolved in 400 g of water Kf= 1.86 Celsius/m and KB = 0.512 Celsius/m. Use 100 degrees Celsius as the boiling point of water

When 20.0 grams of an unknown compound are dissolved in 500. grams of benzene, the freezing point of the resulting solution is 3.77°C. The freezing point of pure benzene is 5.444°C, and the K₁ for benzene is 5.12°C/m. What is the molar mass of the unknown compound? Hint: Round off to two significant digits. O 110 g/mol Ⓒ 120 g/mol O 130 g/mol O 140 g/mol O None of the above

A certain liquid X has a normal boiling point of 142.00 °C and a boiling point elevation constant K = 1.03 °C kg-mol A solution is prepared by dissolving some alanine (C₂H,NO₂) in 550. g of X. This solution boils at 143.2 °C. Calculate the mass of C3H-NO, that was dissolved. Round your answer to 2 significant digits. X S

Ethylene glycol (C₂H₆O₂) is used as an additive to the water in your automobile to lower its freezing point. A solution of ethylene glycol in water has a freezing point of -8.80°C. What is the mole fraction of ethylene glycol in this solution? (Kf for water is 1.86°C･kg/mol). Please use the correct significant figures. Thank you!