The vapour pressure of water is 15.5 mm at 20 °C. The lowering of vapour pressure of 0.02 m K Br solution will be

Which of the following 0.1 M aqueous solutions will exert highest osmotic pressure ?

If equimolar solutions of urea, NaCl, sucrose and $BaC{l}_{2}BaCl\_2$ have boiling points A, B, C and D, then

The molar mass of acetic acid obtained by measuring depression in freezing point is $115.8gmo{l}^{-1}115.8\backslash ,\; gmol^\{-1\}$ . Hence the degree of association is

$\mathrm{\Delta }{T}_b\mathrm{/}m\backslash Delta\; \backslash \; T\_b\; /m$ for NaBr solution will have value $(K_b=0.52Kkgmo{l}^{-1}):(K\_b\; =\; 0.52\; \backslash ,K\; \backslash ,kg\backslash ,\; mol\; ^\{-1\})\; :$

0.2 M urea solution can be isotonic with

The osmotic pressure of 0.1 M HCl solution at 27 °C will be

If a, b, c and d are the van’t Hoff factors for $N{a}_{2}S{O}_{4}Na\_2\; SO\_4$ , glucose and $K_4[Fe(CN{)}_6]K\_4\; [Fe(CN)\_6\; ]$ then

The osmotic pressure of 0.2 M KCl solution at 310 K is

A temperature at which 0.1 M KCl solution will have osmotic pressure 10 atm will be