Similar to the freezing-point depression, the boiling-point elevation deltaT_b o

Question

Similar to the freezing-point depression, the boiling-point elevation deltaT_b of a solution is quantitatively related to the molality m and the boiling-point elevation constant K_b of the solvent by the equation deltaT_b=K_bm where the boiling-point elevation is the difference between the boiling points of the solution and the pure solvent A solution of water (K_b=0512degreesC/m) and glucose boils at 102.06degreesC What is the molal concentration of glucose in this solution? Assume that the boiling point of pure water is 100.00degreesC Express your answer to three significant figures and include the appropriate units.

Explanation / Answer

dTb = iKbm

with,

i = 1

dTb = 102.06 - 100 = 2.06 oC

Kb = 0.512 oC/m

molality will be = 2.06/1 x 0.512 = 4.02 molal

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