vant hoff factor 'i' is greater than 'q' for aqueous solution containing potassium chloride. why?
Answers
Answer:
Oct 15 2019
Van't Hoff factor, I, of a 0.5% (w/w) aqueous solution of KCI which [kf of water =1.86 K kg mol-1, Mol. wt. of KCI=74.5].A.
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Due to dissociation and in presence of a strong electrolyte the Vant Hoff factor 'i' is greater than 'q' for an aqueous solution containing potassium chloride.
Given:
Vant Hoff factor 'i' is greater than 'q' for an aqueous solution containing potassium chloride.
To find:
We are required to find why the Vant Hoff factor 'i' is greater than 'q' for an aqueous solution containing potassium chloride.
Solution:
'i' is the association or dissociation of solute in solution.
Where i = normal molar mass / observed molar mass ---(1)
- If 'i' is greater than 1 then the observed molar mass is lesser than the normal molar mass.
- The observed molar mass is less in case of dissociation
Therefore, Due to dissociation and in presence of a strong electrolyte the Vant Hoff factor 'i' is greater than 'q' for an aqueous solution containing potassium chloride.
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