(B) $\Delta T_{f} = i \times K_{f} \times m$ $\therefore i = \frac{\Delta T_{f}}{K_{f} \times m} = \frac{0.19}{1.86 \times 0.1} = 1.0215 \approx 1.02$

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(B) $\Delta T_{f} = i \times K_{f} \times m$ $\therefore i = \frac{\Delta T_{f}}{K_{f} \times m} = \frac{0.19}{1.86 \times 0.1} = 1.0215 \approx 1.02$ Again from, $\alpha = \frac{i-1}{n-1} = \frac{1.02-1}{2-1} = 0.02$ For $CH_{3}COOH \rightleftharpoons CH_{3}COO^{-} + H^{+}$ $K_{a} = C \alpha^{2}$ $= 0.1 \times (0.02)^{2} = 0.1 \times 4 \times 10^{-4} = 4 \times 10^{-5}$

Class 12 Chemistry Solutions Abnormal molecular mass

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The measured freezing point depression for a $0.1 \ m$ aqueous $CH_{3}COOH$ solution is $0.19^{\circ} C$. The acid dissociation constant $K_{a}$ at this concentration will be (Given, $K_{f}$ the molal cryoscopic constant $= 1.86 \ K \ kg \ mol^{-1}$)

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A
$4.76 \times 10^{-5}$
B
$4 \times 10^{-5}$
C
$8 \times 10^{-5}$
D
$2 \times 10^{-5}$

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$20 \ g$ of a binary electrolyte (molar mass = $100 \ g \ mol^{-1}$) is dissolved in $500 \ g$ of water. The freezing point of the solution is $-0.74 \ ^oC$. Given $K_f = 1.86 \ K \ kg \ mol^{-1}$,the degree of dissociation of the electrolyte is ......... $\%$.

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The measured freezing point depression for a $0.1 \ m$ aqueous $CH_{3}COOH$ solution is $0.19^{\circ} C$. The acid dissociation constant $K_{a}$ at this concentration will be (Given, $K_{f}$ the molal cryoscopic constant $= 1.86 \ K \ kg \ mol^{-1}$)

Similar Questions

At $300 \ K$, the osmotic pressure of a decinormal solution of sodium chloride is $4.82 \ atm$. The degree of dissociation of sodium chloride is $x \times 10^{-2}$. The value of $x$ is $\left(R=0.082 \ L \ atm \ K^{-1} \ mol^{-1}\right)$

The van't Hoff factor for $BaCl_2$ is $2.47$. Calculate the percentage dissociation of $BaCl_2$ in its aqueous solution. (in $\%$)

What is association? What is dissociation?

$0.2$ molal aqueous solution of $KCl$ freezes at $-0.680^{\circ} C$. Calculate van't Hoff factor for this solution. $(K_{f} = 1.86 \ K \ kg \ mol^{-1})$

$20 \ g$ of a binary electrolyte (molar mass = $100 \ g \ mol^{-1}$) is dissolved in $500 \ g$ of water. The freezing point of the solution is $-0.74 \ ^oC$. Given $K_f = 1.86 \ K \ kg \ mol^{-1}$,the degree of dissociation of the electrolyte is ......... $\%$.

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