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

b) Define the isotonic solution. What happens when the blood cell is dipped in a solution containing more than normal saline concentration?

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Solution

a)
$M_{2} = \frac{1000 \times K_{f} \times W_{2}}{Δ T_{f} \times W_{1}}$
$M_{2} = \frac{1000 \times 1.86 \times 18}{(273 - 272.07) \times 200}$

$M_{2} = 180$ g/mol
b)
Isotonic solutions: Two or more solutions exerting the same osmotic pressure are called isotonic solutions. 0.05 M urea solution is isotonic with 0.05 M sucrose solution as both have the same osmotic pressure.
When the blood cell is dipped in a solution containing more than normal saline concentration, it loses water due to osmosis and collapses.

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