Multiple Choice
An ethylene glycol solution contains 25.2 g of ethylene glycol (C2H6O2) in 99.5 mL of water. Determine the change in boiling point. Assume a density of 1.00 g/mL for water.
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13. Solutions
Boiling Point Elevation
Multiple Choice
What is the molality of glucose in an aqueous solution if the boiling point of the solution is 103.15ºC?
A
0.15 m
B
0.29 m
C
6.18 m
D
1.6 m
Verified step by step guidance1
Identify the boiling point elevation formula: ΔT_b = i * K_b * m, where ΔT_b is the boiling point elevation, i is the van't Hoff factor (which is 1 for glucose as it does not ionize), K_b is the ebullioscopic constant of the solvent (water in this case), and m is the molality of the solution.
Calculate the boiling point elevation (ΔT_b) by subtracting the normal boiling point of water (100ºC) from the given boiling point of the solution (103.15ºC).
Use the calculated ΔT_b and the known K_b value for water (0.512 ºC/m) in the boiling point elevation formula to solve for the molality (m).
Rearrange the formula to solve for molality: m = ΔT_b / (i * K_b).
Substitute the values into the rearranged formula to find the molality of the glucose solution.
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