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Depression in Freezing Point

In comparison...

Question

In comparison to a $0.01 M$ solution of glucose, the depression in freezing point of a $0.01 M$ $M g {C l}_{2}$ solution is ?

the same

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about twice

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about three times

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about six times

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Solution

The correct option is C about three times
We have,

$Δ T_{f} = i K_{f} m$ , $i = 1$ for glucose.

$Δ T_{f}^{g l u c o s e} = 1 \times K_{f} \times 0.01$

In case of $M g C l_{2} ⟶ M g^{2 +} + 2 C l^{-}$ , $i = 3$ ,

$Δ T_{f}^{M g C l_{2}} = 3 \times 0.01 \times K_{f}$

$\Rightarrow Δ T_{f}^{M g C l_{2}} = 3 \times Δ T_{f}^{g l u c o s e}$

Hence, the depression in freezing point of $M g C l_{2}$ is $t h r e e t i m e s$ that of glucose.

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In comparison to a 0.01 M solution of glucose, the depression in freezing point of a $0.01 M M g C l_{2}$ solution is ........... .
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In comparison to a 0.01M solution of glucose, the depression in freezing point of a 0.01M MgCl2 solution is ?

The correct option is C about three timesWe have,ΔTf=iKfm, i=1 for glucose.ΔTglucosef=1×Kf×0.01In case of MgCl2⟶Mg2++2Cl−, i=3,ΔTMgCl2f=3×0.01×Kf⇒ΔTMgCl2f=3×ΔTglucosefHence, the depression in freezing point of MgCl2 is three times that of glucose.

In comparison to a $0.01 M$ solution of glucose, the depression in freezing point of a $0.01 M$ $M g {C l}_{2}$ solution is ?