Home
Class 12
CHEMISTRY
Blood freezes at 272.44 K and a solution...

Blood freezes at `272.44 K` and a solution of `3.0 g` of urea in `250 g` of water freezes at `272.63 K`. Calculate the osmotic pressure of blood at `300 K`. (Assume density of blood at `300 K` to be `1 g c c^(-1)`)

Text Solution

Verified by Experts

In this question first calculate `K_(f)` of water from urea solution.
`DeltaT_(f)=K_(f)(((W_(B))/(Mw_(B)))/(W_(A))xx1000)`
`rArrK_(f)=(DeltaT_(f))/(((W_(B))/((Mw_(B))/(W_(A)))xx1000))`
`implies K_(f)=(0.37)/((((3)/(60))/(250)xx1000))=1.85`
`[Delta T_(f)=273-272.63=0.37 K]`
Now determine the molality of blood by using
`DeltaT_(f)=K_(f)m`
Now `DeltaT_(f)=273-272.44=0.56^(@)C`
`m=(DeltaT_(f))/(K_(f))=0.56/1.85=0.303`
`rArrMolarity=molality=0.303`
Now using `pi=CRT`
`rArr pi =0.303xx0.082xx300=7.46 atm`
Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the osmotic pressure of 5% solution of cane sugar (sucrose) at 300 K .

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.

The osmotic pressure of a solution of 3.42 g sugar (molar mass 342) in 500 mL at 300 K will be

0.85% aqueous solution of NaNO_(3) is apparently 90% dissociated . The osmotic pressure of solution at 300 K is

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) )

By dissolving 13.6 g of a substance in 20 g of water, the freezing point decreased by 3.7^(@)C . Calculate the molecular mass of the substance. (Molal depression constant for water = 1.863K kg mol^(-1))

If 1.71 g of sugar (molar mass=342) is dissoved in 500 cm^(3) of a solution at 300K. What will be its osmotic pressure?

6 grams of a substance 'A' dissolved in 100 g of water freezes at - 0.93^(@)C . The molecular mass of 'A' is ( K_(f)=1.86 Km^(-1) ).

A solution containing 18g of non - volatile non - electrolyte solute is dissolved in 200g of water freezes at 272.07K. Calculate the molecular mass of solute. Given K_(f)=1.86kg//mol and freezing point of water = 273K