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  • A 1 molal K4Fe(CN)6 solution has a degree of dissociation of 0.4. Its boiling point is equal to that of another solution which contains 18.1 weight percent of a non-electrolytic solute A. The molar mass of A is __________ u. (Ro

A 1 molal K4Fe(CN)6 solution has a degree of dissociation of 0.4. Its boiling point is equal to that of another solution which contains 18.1 weight percent of a non-electrolytic solute A. The molar mass of A is __________ u. (Round off to the Nearest Integer). [Density of water = 1.0 g cm -3]
 

Answers (1)

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From the below formula, Molar mass can be calculated by morality and given data.

\text { Molality }=\frac{\text { moles of solute }}{\text { kilograms of solvent }}\text { Molality }=\frac{\text { mass of solute }/\textup{Molar mass of solute}}{\text { kilograms of solvent }}

Given,

A 1 molal K4Fe(CN)6 solution has a degree of dissociation of 0.4.

where m is molality.

Effective molality = 0.6 + 1.6 + 0.4 = 2.6m

Now,

A 1 molal K4Fe(CN)6  solution's boiling point is equal to that of another solution which contains 18.1 weight percent of a non-electrolytic solute A. 

So, For the same boiling point, the molality of another solution should also be 2.6 m

Now, 18.1 weight percent solution means 18.1 g solute is present in 100 g solution.

hence, Weight of Solvent water = 100 – 18.1 = 81.9 g

Weight of Solvent water = 81.9/1000 kg

Now, Putting the value.

\text { Molality }=\frac{\text { mass of solute }/\textup{Molar mass of solute}}{\text { kilograms of solvent }}

2.6=\frac{18.1/\textup{M}}{81.9/1000}

So, Molar mass of solute, M = 85.

Ans = 85

Posted by

Kuldeep Maurya

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