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In comparison to a 0.01 M solution of gl...

In comparison to a 0.01 M solution of glucose, the depression in freezing point of a 0.01 M `MgCl_(2)` solution is …….

A

the same

B

about twice

C

about three times

D

about six times

Text Solution

Verified by Experts

The correct Answer is:
C
Explanation : Depression in freezing point is a colligative property. In case of `MgCl_(2)` value of van.t. Hoff factor will be more.
No. of ions yielded when a molecule of `MgCl_(2)` gets dissociated in its aqueous solution is = 3. Thus one molecule of 0.01 M `MgCl_(2)` given out three particles / ions in solution, thereby increasing the number of particles present in its solution to three times.
It is because of this that depression in freezing point of 0.01 M `MgCl_(2)` will be three times as compared to that of 0.01 M - glucose solution, where no dissociation of the molecule takes place.
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  • The freezing point of 0.01 M KCl solution is -2^(@)C . If BaCl_(2) is completely ionized, what is the freezing point of 0.01 M BaCl_(2) solution ?

    A
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    B
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    C
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  • If increase in boiling point of 1 molal glucose solution is 2K increase in freezing point of 2 molal glucose solution is also 2K. Then state the relationship of K_(b) and K_(f) .

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    B
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    C
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