Home
Class 12
CHEMISTRY
A solution was prepared by dissolving 6....

A solution was prepared by dissolving `6.0 g` an organic compound in `100 g` of water. Calculate the osmotic pressure of this solution at `298 K`,when the boiling point of the Solution is `100.2^(@)C`. (`K_(b)` for water =`0.52 K m^(-1)`), R=0.082 L atm `K^(_1) mol^(-1)`)

Text Solution

Verified by Experts

The given values are
`W_("solute")=6.0 g`,`W_("solvent")=100 g`,`K_(b)=0.52 K m^(-1)`
`DeltaT_(b)=100.2-100=0.2`
Now using the formula
`Mw_("solute")=(K_(b)xxW_("solute")xx1000)/(DeltaT_(b)xxW_("solvent"))`
`=(0.52xx6.0xx1000)/(0.2xx100)`
`=156 g mol^(-1)`
Now, `pi=(nRT)/(V)`,`n=W_("solute")/(Mw_("solute"))`
`:.n=6.0/156`
`:. n=(6.0xx0.082xx298)/(156xx0.1)`
`=9.398 atm`
Thus, the osmotic pressure of the solution is `9.398 atm`.
Promotional Banner

Similar Questions

Explore conceptually related problems

A solution of sucrose (molar mass =342) is prepared by dissolving 68.4 g in 1000 g of water. Calculate The osmotic pressure at 273 K.

A solution of sucrose (molar mass =342) is prepared by dissolving 68.4 g in 1000 g of water. Calculate The vapour pressure of solution at 293 K is 0.023atm.

A solution of an organic compound is prepared by dissolving 30 g in 100 g water. Calculate the molecular mass of compound and the osmotic pressure of solution at 300 K , when the elevation in boiling point is 0.52 and K_(b) for water is 0.52 K m^(-1) .

0.2 m aqueous solution of a weak acid (HX) is 20% dissociated. The boiling point of this solution is ( K_(b) for water = 0.52 Km^(-1) )

The osmotic pressure of a solution containing 0.1 mol of solute per litre at 273 K is

A solute containing 0.564g of solute in 36.8g of acetone boils at 56.46^(@)C . Calculate the molar mass of solute if the boiling point of acetone is 56.30^(@)C . [ K_(b) for acetone 1.92K kg. mol^(-1) ]

Calculate the molar mass of a substance 1 g of which when dissolved in 100 g of water gave a solution boiling at 100.1^(@)C at a pressure of 1 atm (K_(b) for water = 0.52 K kg mol^(-1))

A mixture of 0.1 mol of Na_(2)O and 0.1 mol of BaO is dissolved in 1000 g of H_(2)O . Calculate the vapour pressure of solution at 373 K .

Calculate the osmotic pressure of 0.05% urea solution in water at 20^(@) C. Given R = 0.0821 atm mol^(-1)K^(-1) . Molar mass of urea = 60 g mol^(-1) .