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38 solutions

Boiling Point Elevation

Q. When 8.19 g of an unknown non-electrolyte is dissolved in 50.0 g of carbon tetrachloride, the boiling point increased by 2.61 degrees C. If the Kbp of the solvent is 4.95 K/m, calculate the molar mass of the unknown solute.

Solved • Jan 22, 2020

Boiling Point Elevation

Q. Calculate the boiling point (in degrees C) of a solution made by dissolving 7.23 g of urea {CO(NH 2 ) 2 } in 90.6 g of water. The Kbp of the solvent is 0.512 K/m and the normal boiling point is 373 K. Enter your answer to 2 decimal places.

Solved • Jan 22, 2020

Boiling Point Elevation

Q. Calculate the boiling point (in degrees C) of a solution made by dissolving 5.43 g of fructose (C6H12O6) in 35.4 g of acetone. The Kbp of the solvent is 1.71 K/m and the normal boiling point is 56.2 degrees C. Enter your answer to 2 decimal places.

Solved • Jan 22, 2020

Boiling Point Elevation

Q. When 5.46 g of an unknown non-electrolyte is dissolved in 50.0 g of water, the boiling point increased to 100.645 degrees C from 100 degrees C. If the Kbp of the solvent is 0.512 K/m, calculate the molar mass of the unknown solute.

Solved • Jan 22, 2020

Boiling Point Elevation

Q. Determine the boiling point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (d = 0.877 g/mL). Pure benzene has a boiling point of 80.1°C and a boiling point depression constant of 2.53°C/m. A) 82.3°C B) 2.2°C C) 80.4°C D) 82.6°C E) 2.5°C

Solved • Jul 15, 2019

Boiling Point Elevation

Q. A glucose solution contains 54.8g of glucose (C6H12O6) in 495 g of water. Compute the freezing point and boiling point of the solution. (Assume density of 1.00g/mL for water.)

Solved • Dec 4, 2019

Boiling Point Elevation

Q. A solution of water (Kb=0.512 ∘C/m) and glucose boils at 101.56 ∘C. What is the molal concentration of glucose in this solution? Assume that the boiling point of pure water is 100.00 ∘C. Express your answer to three significant figures and include the appropriate units.

Solved • Nov 12, 2019