Calculate the osmotic pressure of 0.03 mole of non electrolyte solute dissolved in $0.1 \mathrm{dm}^3$ of water at $300 \mathrm{~K} .\left[\mathrm{R}=0.082 \mathrm{dm}^3 \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right]$

Identify from following salts so that the solubility of salt in water decreases with increase in temperature.

Calculate the molal elevation constant of solvent if boiling point of 0.12 m solution is 319.8 K (Boling point of solvent $=319.5 \mathrm{~K}$ )

Calculate the concentration of an aqueous solution of non electrolyte at 300 K if its osmotic pressure is 12 atm .

$$ \left[\mathrm{R}=0.0821 \mathrm{~atm} \mathrm{dm}^3 \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right] $$