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Question

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


A
the same
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B
about twice
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C
about three times
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D
about six times
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Solution

The correct option is C about three times
We have,

$$\Delta T_f = i K_f m$$, $$i =1$$ for glucose.

$$\Delta T_f ^{glucose}= 1\times K_f \times 0.01$$

In case of $$MgCl_2\longrightarrow Mg^{2+}+ 2Cl^-$$, $$i= 3$$,

$$\Delta T_f ^{MgCl_2}= 3\times 0.01\times K_f$$

$$\Rightarrow \Delta T_f^{MgCl_2}= 3\times \Delta T_f^{glucose}$$

Hence, the depression in freezing point of $$MgCl_2$$ is $$three\ times$$ that of glucose. 


Chemistry

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