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  • (a)    Define the following terms :         (i)    Ideal solution        (ii)    Osmotic pressure. <p

(a)    Define the following terms :
        (i)    Ideal solution
       (ii)    Osmotic pressure.

(b)    Calculate the boiling point elevation for a solution prepared by adding 10 g CaCl2 to 200 g of water, assuming that CaCl2 is completely dissociated. (Kb for water = 0.512 K kgmol–1 ; Molar mass of CaCl2 = 111 g mol–1 )

 

 

 

 
 
 
 
 

Answers (1)

(a)    (i)    Ideal Solution is a solution of two liquids if it obeys Raoult's law in solution i.e \mathrm{P_1 = P_1^o\chi_1; \ P_2 = P_2^o\chi_2; P_T = P_1^o\chi_1 + P_2^o\chi_2; \Delta H_{mix} = 0}, no heat is evolved or absorbed during the formation of solution.

\mathrm{\Delta V_{mix} = 0}, Volume remains unchanged on mixing.

       (ii)    Osmotic Pressure is the extra pressure which has to be applied on the solution side so as to just stop osmosis.

(b)    \mathrm{\Delta T_b = ?\qquad \Delta T_b = iK_bm}

        \mathrm{K_b = 0.5.12 \ K \ kg \ mol^{-1}}

        Molar mass of CaCl2 = 111 gmol-1

        \mathrm{i = 3}    (complete dissociation)

        \mathrm{m = \frac{10}{111}\times \frac{1000}{200} = 0.450}

        \mathrm{\Delta T_b = 3\times 0.512\times 0.450 = 0.6918K}

Posted by

Sumit Saini

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