Calculate osmotic pressure exerted by a solution containing $$0.822 \mathrm{~g}$$ of solute in $$300 \mathrm{~mL}$$ of water at $$300 \mathrm{~K}$$.

(Molar mass of solute $$=340 \mathrm{~g} \mathrm{~mol}^{-1}, \mathrm{R}=0.0821 \mathrm{~L} \mathrm{~atm} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$$)

The pH of monoacidic weak base is 10.9. Calculate the percent dissociation in 0.02 M solution.

Lithium shows diagonal relationship with

How many molecules of ammonia gas are present in 67.2 dm$$^3$$, measured at S.T.P.?