(B) The dissociation of the weak acid is given by: $HX \rightleftharpoons H^+ + X^-$. Since the degree of dissociation $\alpha = 0.20$,the van't Hoff

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(B) The dissociation of the weak acid is given by: $HX \rightleftharpoons H^+ + X^-$. Since the degree of dissociation $\alpha = 0.20$,the van't Hoff factor $i = 1 + \alpha(n-1) = 1 + 0.20(2-1) = 1.2$. The depression in freezing point is calculated as $\Delta T_f = i \times K_f \times m$. Substituting the values: $\Delta T_f = 1.2 \times 1.86 \times 0.5 = 1.116 \ K \approx 1.12 \ K$.

Class 12 Chemistry Solutions Colligative properties of electrolyte

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$A$ $0.5 \ m$ aqueous solution of a weak acid $(HX)$ is $20\%$ ionized. If $K_f$ for water is $1.86 \ K \ kg \ mol^{-1}$,the depression in freezing point of the solution is ....... $K$.

A
$0.56$
B
$1.12$
C
$0.28$
D
$0.84$

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Colligative properties of electrolyte

The depression in freezing point of a $NaCl$ solution is $6 \ K$. If $K_f = 1.86 \ K \ kg \ mol^{-1}$ for water,then the amount of $NaCl$ dissolved in $1 \ kg$ of water is ............. $mol$?

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$2 \ m$ aqueous solution of an electrolyte $X_3Y_2$ is $25\%$ ionized. The boiling point of the solution is .......... $K.$ ($K_b$ for $H_2O = 0.52 \ K \ kg/mol$)

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Which of the following $0.1 \ m$ aqueous solutions exhibits the highest osmotic pressure at $25^{\circ}C$?

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Which of the following will have the lowest vapor pressure?

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The freezing point (in ${}^{\circ}C$) of a solution containing $0.1 \ g$ of $K_3[Fe(CN)_6]$ (Mol. Wt. $329$) in $100 \ g$ of water $(K_f = 1.86 \ K \ kg \ mol^{-1})$ is

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$A$ $0.5 \ m$ aqueous solution of a weak acid $(HX)$ is $20\%$ ionized. If $K_f$ for water is $1.86 \ K \ kg \ mol^{-1}$,the depression in freezing point of the solution is ....... $K$.

Similar Questions

The depression in freezing point of a $NaCl$ solution is $6 \ K$. If $K_f = 1.86 \ K \ kg \ mol^{-1}$ for water,then the amount of $NaCl$ dissolved in $1 \ kg$ of water is ............. $mol$?

$2 \ m$ aqueous solution of an electrolyte $X_3Y_2$ is $25\%$ ionized. The boiling point of the solution is .......... $K.$ ($K_b$ for $H_2O = 0.52 \ K \ kg/mol$)

Which of the following $0.1 \ m$ aqueous solutions exhibits the highest osmotic pressure at $25^{\circ}C$?

Which of the following will have the lowest vapor pressure?

The freezing point (in ${}^{\circ}C$) of a solution containing $0.1 \ g$ of $K_3[Fe(CN)_6]$ (Mol. Wt. $329$) in $100 \ g$ of water $(K_f = 1.86 \ K \ kg \ mol^{-1})$ is

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