(A) The elevation in boiling point is given by $\Delta T_b = i \times K_b \times m$. Here,$\Delta T_b = 100\,^oC - 95\,^oC = 5\,K$. For $NaCl$,the van

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(A) The elevation in boiling point is given by $\Delta T_b = i \times K_b \times m$. Here,$\Delta T_b = 100\,^oC - 95\,^oC = 5\,K$. For $NaCl$,the van't Hoff factor $i = 1 + \alpha = 1 + 0.9 = 1.9$. The molality $m = \frac{w}{M \times W_{solvent(kg)}}$,where $w$ is the mass of $NaCl$ and $M = 58.5\,g/mol$. Substituting the values: $5 = 1.9 \times 0.52 \times \frac{w}{58.5 \times 1}$. Solving for $w$: $w = \frac{5 \times 58.5}{1.9 \times 0.52} = \frac{292.5}{0.988} \approx 296.05\,g$.

Class 12 Chemistry Solutions Colligative properties of electrolyte

Medium

At higher altitude,the boiling point of water is $95\,^oC$. The amount of $NaCl$ added to $1\, kg$ of water $(K_b = 0.52\, K\, kg\, mol^{-1})$ in order to raise the boiling point of the solution to $100\,^oC$ is ......... $g$. (Assuming $90\%$ ionization of $NaCl$)

A
$296.05$
B
$281.25$
C
$270$
D
$310$

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Colligative properties of electrolyte

$A$ $0.2 \, m$ aqueous solution of a weak acid $(HX)$ is $20 \% $ ionised. The freezing point of this solution is .............. $^o C$ (Given ${K_f} = 1.86 \, ^o C/m$ for water)

MediumIIT 1995

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The freezing point of a $1.00 \ m$ aqueous solution of $HF$ is found to be $-1.91 \ ^oC$. The freezing point constant of water,$K_f$ is $1.86 \ K \ kg \ mol^{-1}$. The percentage dissociation of $HF$ at this concentration is ................ $\%$

DifficultAIEEE 2012

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Which of the following solutions has an osmotic pressure nearest to that of an equimolar solution of $K_4[Fe(CN)_6]$?

Medium

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At a constant temperature,the vapor pressures of aqueous solutions of $Na_2SO_4$,urea,$AlCl_3$,and $1.2 \, m \, KCl$ are approximately equal. The molalities of the aqueous solutions of $Na_2SO_4$,urea,and $AlCl_3$ are,respectively: (Assume $100 \%$ dissociation of the solute)

Medium

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Which of the following salts has the same value of Van't Hoff factor $i$ as that of $K_4[Fe(CN)_6]$?

EasyAIPMT 1994

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At higher altitude,the boiling point of water is $95\,^oC$. The amount of $NaCl$ added to $1\, kg$ of water $(K_b = 0.52\, K\, kg\, mol^{-1})$ in order to raise the boiling point of the solution to $100\,^oC$ is ......... $g$. (Assuming $90\%$ ionization of $NaCl$)

Similar Questions

$A$ $0.2 \, m$ aqueous solution of a weak acid $(HX)$ is $20 \% $ ionised. The freezing point of this solution is .............. $^o C$ (Given ${K_f} = 1.86 \, ^o C/m$ for water)

The freezing point of a $1.00 \ m$ aqueous solution of $HF$ is found to be $-1.91 \ ^oC$. The freezing point constant of water,$K_f$ is $1.86 \ K \ kg \ mol^{-1}$. The percentage dissociation of $HF$ at this concentration is ................ $\%$

Which of the following solutions has an osmotic pressure nearest to that of an equimolar solution of $K_4[Fe(CN)_6]$?

At a constant temperature,the vapor pressures of aqueous solutions of $Na_2SO_4$,urea,$AlCl_3$,and $1.2 \, m \, KCl$ are approximately equal. The molalities of the aqueous solutions of $Na_2SO_4$,urea,and $AlCl_3$ are,respectively: (Assume $100 \%$ dissociation of the solute)

Which of the following salts has the same value of Van't Hoff factor $i$ as that of $K_4[Fe(CN)_6]$?

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