A 0.97 m aqueous solution of an ionic compound with the formula MX has a freezing point of -2.7 ∘C . a) Calculate the van't Hoff factor (i) for MX at this concentration.
A 0.97 m aqueous solution of an ionic compound with the formula MX has a freezing point of -2.7 ∘C . a) Calculate the van't Hoff factor (i) for MX at this concentration.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A 0.97 m aqueous solution of an ionic compound with the formula MX has a freezing point of -2.7 ∘C .
a) Calculate the van't Hoff factor (i) for MX at this concentration.
Expert Solution
Step 1 depression in freezing point
and molality (m) relation is
= i x Kf x m
where
= depression in freezing point
= To - Ts = 0 oC - (-2.7 oC) = 2.7oC
i = van't Hoff factor = ? (for 100% dissociation)
m = molality of solution = 0.97 m
Kf = molal freezing point constant of water = 1.86 oC/m
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