For 0.01 , M solutions of urea, common salt ( | vedclass

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(C) The depression of freezing point $(\Delta T_f)$ is given by the formula $\Delta T_f = i 	imes K_f 	imes m$, where $i$ is the van't Hoff factor.S

Vedclass · Accepted Answer

$1 : 2 : 3$

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(C) The depression of freezing point $(\Delta T_f)$ is given by the formula $\Delta T_f = i 	imes K_f 	imes m$, where $i$ is the van't Hoff factor.Since the molality $(m)$ and the freezing point depression constant $(K_f)$ are the same for all solutions, the ratio of $\Delta T_f$ is equal to the ratio of their van't Hoff factors $(i)$.For urea (a non-electrolyte), $i = 1$.For common salt $(NaCl)$, it dissociates as $NaCl ightarrow Na^+ + Cl^-$, so $i = 2$.For $Na_2SO_4$, it dissociates as $Na_2SO_4 ightarrow 2Na^+ + SO_4^{2-}$, so $i = 3$.Therefore, the ratio of depression of freezing point is $1 : 2 : 3$.

For $0.01 \, M$ solutions of urea, common salt $(NaCl)$, and $Na_2SO_4$, the ratio of depression of freezing point is:

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For $0.01 \ M$ solutions of urea,$NaCl$,and $Na_2SO_4$,the ratio of their depression in freezing point is .......

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