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
B
about twice
C
about three times
D
about six times

Solution

The correct option is C about three timesWe 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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