At `10^(@)` C, the average osmotic pressure of blood is 8.8 atm. Find the concentration of the various constituents in the blood. Assuming that the concentration is the same as the molarity. Find the freezing point of the solution `(K_(f) " for water " = 1.86 K" kg mol"^(-1))`

Explanation

Step - I : Calrulation for concencertration of the solution.
According to Van.t Hoff equation
`pi = "CRT" or C = (pi)/(RT)`
`pi = 8.8 "atm" , T = 40^(@) C = 313 K `
R = 0.0821 L atm `K^(-1) mol^(-1)`
C = `(8.8)/(0.0821 xx 313) = 0.34 "molL"^(-1) `(M)
Step -II : Calculation of freezing point of the solution Depression in free.zing point of solution
`Delta T_(f) = K_(f) xx m`
m = 0.34 mol `Kg^(-1) ` (same as molarity as given)
`K_(f) = 1.86 K" kg mol"^(-1)`
`Delta T_(f) = 1.86 xx 0.34 (because Delta T_(f) = K_(f) m) `
= 0.63 K = `0.63^(@)` C
Freezing point of the solution = 0 `0.63^(@) ` C
= - `0.63^(@)` C