Question

An aqueous solution containing 4.9gram of a solute dissolved in 500ml of solutions shows an osmotic pressure of 2.1 atmosphere at 27°C. What is the nature of the solute, if the molar mass of the solute is 57.4amu ?​

Answer 1

The nature of the solute is associating.

Explanation:

$\pi =iCRT$

$\pi$ = osmotic pressure  = 2.1 atm

i = vant hoff factor

C= concentration in Molarity  

R= solution constant  = 0.0821 Latm/Kmol

T= temperature = $27^0C=(27+273)K=300K$

$Molarity=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{volume of solution in ml}}$

$Molarity=\frac{4.9\times 1000}{57.4\times 500}=0.17M$

$2.1=i\times 0.17\times 0.0821\times 300$

$i=0.5=\frac{1}{2}$

Thus as the vant hoff factor is less than 1, the solute undergoes association.

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