A solution is prepared by dissolving 0.6 g of urea (molar mass $=60\mathrm{ }\mathrm{g}\mathrm{ }\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$) and $1.8\mathrm{ }\mathrm{g}$ of glucose (molar mass $=180\mathrm{ }\mathrm{g}\mathrm{ }\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$) in 100 mL of water at ${27}^{\mathrm{o}}\mathrm{C}.$ The osmotic pressure of the solution is:
($\mathrm{R}=0.08206\mathrm{ }\mathrm{L}$$\text{atm}$ ${\mathrm{K}}^{-1}\mathrm{ }\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$)

Determination of the molar mass of acetic acid in benzene using freezing point depression is affected by:

If $80 \mathrm{g}$ of copper sulphate ${\mathrm{CuSO}}_4·5{\mathrm{H}}_2\mathrm{O}$ is dissolved in deionised water to make $5 \mathrm{L}$ of solution. The concentration of the copper sulphate solution is $x\times {10}^{-3}\text{ mol }{L}^{-1}.$ The value of $x$ is _____.

$[\text{Atomic masses }\mathrm{Cu} : 63.54\mathrm{u}, \mathrm{S} : 32\mathrm{u}, \mathrm{O} : 16\mathrm{u}, \mathrm{H} : 1\mathrm{u}]$