The average osmotic pressure of human blood is 7.7 atm at `40^(@)C` .
(a) What would be the total concentrationn of various solutes in the blood ?
(b) Assuming the concentration to be essentially the same as the molality , calculate the freezing point of blood (`k_(f)` for water `= 1.86^(@)C m^(-1)`).

Answer

`0.30 mol L^(-1) , -0.558^(@)C`

Explanation

`c = (pi)/(RT) = (7.7)/(0.0821 xx 313) = 0.30 mol L^(-1)`
Assuming molar concentration as equal to molality
`m = 0.30, k_(f) = 1.86^(@)C m^(-1)`
`Delta T_(f) = k_(f) xx m = 1.86 xx 0.30 = 0.558^(@)`
Freezing point of blood ` = 0-0.558`
` = - 0.558^(@)C`