The osmotic pressure ofa solution containing 50 g of a solute in one litre of solution at 300K is 20.5 atmosphere. Calculate the molecular mass of the solute.

Explanation

Given, osmotic pressure (x) = 20.5 atm
Volume of solution (V) - 1L
Mass of solute (wo) = 50 g
Temperature - 300 K
Gas constant (R)=0.082 L atm `K^(-1)mol^(-1)`
To find, molar mass of solute `(M_B)` = ?
Relation used :
`pi=CRT`
`pi=(W_BxxRT)/(M_BxxV)`
`pi=(50xx0.082xx300)/(M_Bxx1)`
or `M_B=(50xx0.082xx300xx1)/(20.5)`
`M_B=60.00`
Thus, molecular mass of solute = 60.00 g/mol