If the 3.90 m solution from Part A boils at 103.45 ∘C, what is the actual value of the van't Hoff factor, i? The boiling point o

Question

schepotkina

3 months ago

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If the 3.90 m solution from Part A boils at 103.45 ∘C, what is the actual value of the van't Hoff factor, i? The boiling point o

f pure water is 100.00 ∘C and Kb is equal to 0.512 ∘C/m.

Chemistry

1 answer:

alisha [2.9K] · Answer 1 · 2026-02-25T12:49:50+03:00

<span>Some solutions demonstrate colligative properties, which rely on the quantity of solute in a solvent. To find the elevation in boiling point, we use the formula:

</span><span>ΔT(boiling point) = (Kb)mi

where Kb represents a constant, m is the solution's molality, and i is the van't Hoff factor.

From the provided information, we can easily determine i as follows:

</span>ΔT(boiling point) = (Kb)mi
103.45 - 100 = (0.512)3.90i
i = 1.73 <-------van't Hoff factor