If compound dissociates in solvent $$i > 1$$  and on association $$i < 1.$$

When we mix $${C_2}{H_5}I$$  and $${C_2}{H_5}OH,$$   there is change in enthalpy and volume, so it is an example of non-ideal solution.

It is capillary action.

$$\eqalign{ & {M_1}{V_1} = {M_2}{V_2};0.02\,M \times 4\,L = {M_2} \times 5\,L \cr & {M_2} = \frac{{0.02 \times 4}}{5} = 0.016\,M \cr} $$
Here, molality will be equal to molarity as for $$NaCl,$$  molecular weight is equal to its equivalent weight.

$$\eqalign{ & \pi = iCRT = i\frac{n}{V}RT \cr & n = \frac{{\pi \times V}}{{i \times R \times T}} \cr & \,\,\, = \frac{{0.5 \times 2}}{{2.47 \times 0.0821 \times 300}} \cr & \,\,\, = 0.0164\,\,mol \cr & {\text{Amount of}}\,\,CaC{l_2} = n \times M = 0.0164 \times 111 = 1.820\,g \cr} $$

Mercury is non-volatile.

$$\eqalign{ & {\text{Number of moles of urea}} = \frac{{120}}{{60}} = 2 \cr & {\text{Total mass of solution = 1000 + 120 = 1120}}g \cr & {\text{Total volume of solution (in L) = }}\frac{{Mass}}{{Density}} \cr & = \frac{{1120}}{{1.15 \times {{10}^3}}} = \frac{{112}}{{115}}L \cr & {\text{Molarity of the solution}} = \frac{{{\text{Number}}\,{\text{of}}\,{\text{moles}}}}{{{\text{Volume}}\,{\text{in}}\,{\text{L}}}} \cr & = \frac{{2 \times 115}}{{112}} = 2.05\,mol\,{L^{ - 1}} \cr} $$

Higher the value of $${K_H},$$  lower is the solubility of gas in the liquid.

$$PQ$$  corresponds to increase in vapour pressure of solvent with temperature and $$XY$$  corresponds to increase in vapour pressure of solution with temperature. $$\Delta T$$  is the elevation in boiling point of a solution.

If we plot a graph between the vapour pressure and the temperature. We would get a curve that rises faster as $$T$$ increases, giving a curved line